Chemistry Final Exam 2023
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Chapter 18 #1 - 19., Ch 17 20-40
Last updated 6:37 PM on 7/20/23
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1
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Determine the effect on the following equilibrium if the partial pressure of oxygen is decreased.
2H2S(g) + O2(g) ⟷ 2S(s) + 2H2O(g)
\
The equilibrium will shift left.
Increase in the partial pressure of water and hydrogen sulfide gas would result.
No effect on the equilibrium.
A decrease in the partial pressure of water and hydrogen sulfide gas would result.
The equilibrium will shift right.
2H2S(g) + O2(g) ⟷ 2S(s) + 2H2O(g)
\
The equilibrium will shift left.
Increase in the partial pressure of water and hydrogen sulfide gas would result.
No effect on the equilibrium.
A decrease in the partial pressure of water and hydrogen sulfide gas would result.
The equilibrium will shift right.
The equilibrium will shift left.
* the products will try to compensate for the decreased partial pressure of oxygen is decreased.
* favors the reactants
* the products will try to compensate for the decreased partial pressure of oxygen is decreased.
* favors the reactants
2
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Predict the effect if the partial pressure of PCl5(g) is increased using the following equation.
PCl3(g) +Cl2(g)⟶ PCl5(g)
No effect.
Shift right.
A decrease in partial pressure of phosphorous trichloride and phosphorous pentachloride.
\
Shift left.
An increase in partial pressure of phosphorous trichloride and phosphorous pentachloride.
PCl3(g) +Cl2(g)⟶ PCl5(g)
No effect.
Shift right.
A decrease in partial pressure of phosphorous trichloride and phosphorous pentachloride.
\
Shift left.
An increase in partial pressure of phosphorous trichloride and phosphorous pentachloride.
No efffect
* the arrow isn’t double
* the arrow isn’t double
3
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Which variables would not effect the following equilibrium?
CH4(g) + 2O2(g) ⟷ CO2(g) + 2H2O(g)
Increase in total pressure.
Increase in partial pressure of CO2(g).
Increase in partial pressure of O2(g).
Increase in partial pressure of CH4(g).
Decrease in partial pressure of H2O(g).
CH4(g) + 2O2(g) ⟷ CO2(g) + 2H2O(g)
Increase in total pressure.
Increase in partial pressure of CO2(g).
Increase in partial pressure of O2(g).
Increase in partial pressure of CH4(g).
Decrease in partial pressure of H2O(g).
Increase in total pressure.
* the amount of moles on each side is equal
* the amount of moles on each side is equal
4
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How is this reaction sequence regulated?
CO2(g) + H2O(l) ⟷ H2CO3(aq)
H2CO3(aq) ⟷ H+1(aq) + HCO3-1(aq)
Breathing controls carbon dioxide concentration and carbonic anhydrase catalyzes the reaction to lower the activation energy.
Ingestion of nutrients controls carbon dioxide concentration and carbonic anhydrase catalyzes the reaction to lower the activation energy.
Metabolism controls carbon dioxide concentration and carbonic anhydrase catalyzes the reaction to increase the activation energy.
Ingestion of nutrients controls carbon dioxide concentration and carbonic anhydrase catalyzes the reaction to increase the activation energy.
Breathing controls carbon dioxide concentration and carbonic anhydrase catalyzes the reaction to increase the activation energy.
CO2(g) + H2O(l) ⟷ H2CO3(aq)
H2CO3(aq) ⟷ H+1(aq) + HCO3-1(aq)
Breathing controls carbon dioxide concentration and carbonic anhydrase catalyzes the reaction to lower the activation energy.
Ingestion of nutrients controls carbon dioxide concentration and carbonic anhydrase catalyzes the reaction to lower the activation energy.
Metabolism controls carbon dioxide concentration and carbonic anhydrase catalyzes the reaction to increase the activation energy.
Ingestion of nutrients controls carbon dioxide concentration and carbonic anhydrase catalyzes the reaction to increase the activation energy.
Breathing controls carbon dioxide concentration and carbonic anhydrase catalyzes the reaction to increase the activation energy.
Breathing controls carbon dioxide concentration and carbonic anhydrase catalyzes the reaction to lower the activation energy.
5
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Which of the following explains the term "dynamic" as applied to chemical equilibrium?
The reaction stops when equilibrium is reached.
Reactants can form products until equilibrium is established.
The reaction continues to convert reactants to products, and products to reactants when the reaction rates are equal, but with no net change in concentration at equilibrium.
Products can form reactants until equilibrium is established.
The reaction continues to convert reactants to products, and products to reactants when the concentrations are equal , but with no net change in concentration at equilibrium.
The reaction stops when equilibrium is reached.
Reactants can form products until equilibrium is established.
The reaction continues to convert reactants to products, and products to reactants when the reaction rates are equal, but with no net change in concentration at equilibrium.
Products can form reactants until equilibrium is established.
The reaction continues to convert reactants to products, and products to reactants when the concentrations are equal , but with no net change in concentration at equilibrium.
The reaction continues to convert reactants to products, and products to reactants when the reaction rates are equal, but with no net change in concentration at equilibrium.
6
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Which kinetic factor involves the total energy required for bond formation?
\
Temperature
Concentration
Total Pressure
State
Partial Pressure
\
Temperature
Concentration
Total Pressure
State
Partial Pressure
Temperature
7
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What type of reaction and how much energy is involved in a reaction of silicon tetrachloride with water?
SiO2(s) +4HCl(g) ⟷ SiCl4(g) + 2H2O(g) ΔH= +139.5 kJ/mole
\
Endothermic with ΔH = -139.5 kJ/mole.
Exothermic with ΔH = +139.5 kJ/mole.
Exothermic with ΔH = -139.5 kJ/mole.
Endothermic with ΔH = +139.5 kJ/mole.
Exothermic with ΔH = -0.007168 kJ/mole.
SiO2(s) +4HCl(g) ⟷ SiCl4(g) + 2H2O(g) ΔH= +139.5 kJ/mole
\
Endothermic with ΔH = -139.5 kJ/mole.
Exothermic with ΔH = +139.5 kJ/mole.
Exothermic with ΔH = -139.5 kJ/mole.
Endothermic with ΔH = +139.5 kJ/mole.
Exothermic with ΔH = -0.007168 kJ/mole.
Exothermic with ΔH = -139.5 kJ/mole.
8
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Which combination in the following equation creates a buffer?
H2PO4-1(aq) + NH3(aq) ⟷ NH4+1(aq) + HPO4-2(aq)
\
NH3(aq) is the acid, NH4+1(aq) is the conjugate base.
NH4+1(aq) is the acid, NH3(aq) is the conjugate base.
H2PO4-1(aq) is an acid, HPO4-2(aq) is the conjugate base.
H2PO4-1(aq) is the base, HPO4-2(aq) is the conjugate acid.
HPO4-2(aq) is the base, H2PO4-1(aq) is the conjugate acid.
H2PO4-1(aq) + NH3(aq) ⟷ NH4+1(aq) + HPO4-2(aq)
\
NH3(aq) is the acid, NH4+1(aq) is the conjugate base.
NH4+1(aq) is the acid, NH3(aq) is the conjugate base.
H2PO4-1(aq) is an acid, HPO4-2(aq) is the conjugate base.
H2PO4-1(aq) is the base, HPO4-2(aq) is the conjugate acid.
HPO4-2(aq) is the base, H2PO4-1(aq) is the conjugate acid.
H2PO4-1(aq) is an acid, HPO4-2(aq) is the conjugate base.
9
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Which of the following is true about blood pH regulation?
\
The bicarbonate buffer and phosphate buffer systems neutralize excess acid, blood soluble proteins are subsequently used as a buffer.
The bicarbonate buffer and phosphate buffer systems neutralize excess acid, with the kidney acting as a final hydrogen ion filter.
The bicarbonate buffer system neutralizes excess acid, blood soluble proteins are subsequently used as a buffer, with the kidney acting as a final hydrogen ion filter.
The bicarbonate buffer and phosphate buffer systems neutralize excess acid, blood soluble proteins are subsequently used as a buffer, with the liver secreting bile salts as a final buffering mechanism.
The bicarbonate buffer and phosphate buffer systems neutralize excess acid, blood soluble proteins are subsequently used as a buffer, with the kidney acting as a final hydrogen ion filter.
\
The bicarbonate buffer and phosphate buffer systems neutralize excess acid, blood soluble proteins are subsequently used as a buffer.
The bicarbonate buffer and phosphate buffer systems neutralize excess acid, with the kidney acting as a final hydrogen ion filter.
The bicarbonate buffer system neutralizes excess acid, blood soluble proteins are subsequently used as a buffer, with the kidney acting as a final hydrogen ion filter.
The bicarbonate buffer and phosphate buffer systems neutralize excess acid, blood soluble proteins are subsequently used as a buffer, with the liver secreting bile salts as a final buffering mechanism.
The bicarbonate buffer and phosphate buffer systems neutralize excess acid, blood soluble proteins are subsequently used as a buffer, with the kidney acting as a final hydrogen ion filter.
The bicarbonate buffer and phosphate buffer systems neutralize excess acid, blood soluble proteins are subsequently used as a buffer, with the kidney acting as a final hydrogen ion filter.
10
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Which of the following describes the variable influenced by activation energy on reaction rates?
\
Particle orientation
Particle proximity
Particle surface area
Particle density
Particle velocity
\
Particle orientation
Particle proximity
Particle surface area
Particle density
Particle velocity
Particle orientation
11
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Using the following chemical equations, determine how the equilibrium will be affected if pH is increased?
CO2(g) + H2O(l) ⟷ H2CO3(aq)
H2CO3(aq) ⟷ H+1(aq) + HCO3-1(aq)
\
More CO2(g) and more HCO3-1(aq) will be produced.
There will be no effect on the equilibrium.
More H+1(aq) will be produced and the HCO3-1(aq) concentration will increase.
More CO2(g) will be produced.
Less CO2(g) will be produced and the HCO3-1(aq) concentration will decrease.
CO2(g) + H2O(l) ⟷ H2CO3(aq)
H2CO3(aq) ⟷ H+1(aq) + HCO3-1(aq)
\
More CO2(g) and more HCO3-1(aq) will be produced.
There will be no effect on the equilibrium.
More H+1(aq) will be produced and the HCO3-1(aq) concentration will increase.
More CO2(g) will be produced.
Less CO2(g) will be produced and the HCO3-1(aq) concentration will decrease.
More H+1(aq) will be produced and the HCO3-1(aq) concentration will increase.
12
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Which of the following could generate a buffer with a strong base?
\
Hydrochloric acid
Hydrobromic acid
Perchloric acid
**Nit**ric acid
Acetic acid
\
Hydrochloric acid
Hydrobromic acid
Perchloric acid
**Nit**ric acid
Acetic acid
Acetic acid
\
* weak acid and a strong base can make a buffer
\
* weak acid and a strong base can make a buffer
13
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Which of the following is the primary biological mechanism for controlling pH?
\
Phosphate buffer
Blood plasma
The kidney
Amino acids in blood soluble protiens
Bicarbonate buffer
\
Phosphate buffer
Blood plasma
The kidney
Amino acids in blood soluble protiens
Bicarbonate buffer
Bicarbonate buffer
14
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Which of the following is a biological catalyst?
RNA
Enzymes
DNA
Lipids
Carbohydrates
RNA
Enzymes
DNA
Lipids
Carbohydrates
Enzymes
15
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Predict the effect on the equilibrium if HBr is removed using the following equation?
HBr + AgOH ⟷ AgBr + H2O
\
This equation does not represent an equilibrium system.
Both reactants and products would be produced.
Neither reactant or products would be produced.
Shift right.
Shift left.
HBr + AgOH ⟷ AgBr + H2O
\
This equation does not represent an equilibrium system.
Both reactants and products would be produced.
Neither reactant or products would be produced.
Shift right.
Shift left.
Shift left
* since the reactants are decreased the equilibrium will favor the reactants
* since the reactants are decreased the equilibrium will favor the reactants
16
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Define chemical equilibrium.
The reaction rate in the forward direction equals the reaction rate in the reverse direction resulting in a continuous reaction with no net change.
The concentration of the reactants equals the concentration of the products resulting in a continuous reaction with no net change.
The chemical reactions stops when the concentration of reactants and the forward reactions rate equals the concentration of the products and the reverse reaction rate.
The chemical reaction stops when the concentration of the reactants equals the concentration of the products.
The chemical reaction stops when the reaction rate in the forward direction equals the reaction rate in the reverse direction.
The reaction rate in the forward direction equals the reaction rate in the reverse direction resulting in a continuous reaction with no net change.
The concentration of the reactants equals the concentration of the products resulting in a continuous reaction with no net change.
The chemical reactions stops when the concentration of reactants and the forward reactions rate equals the concentration of the products and the reverse reaction rate.
The chemical reaction stops when the concentration of the reactants equals the concentration of the products.
The chemical reaction stops when the reaction rate in the forward direction equals the reaction rate in the reverse direction.
The reaction rate in the forward direction equals the reaction rate in the reverse direction resulting in a continuous reaction with no net change.
17
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Which of the following chemical kinetic (reaction rates) factors in biological systems results in a more efficient system?
Lower body temperature.
Solid state of cells.
Large cell size.
Decreased activation energy.
Liquid state of cells.
Lower body temperature.
Solid state of cells.
Large cell size.
Decreased activation energy.
Liquid state of cells.
Decreased activation energy.
18
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What is the effect of equilibrium when heat is removed (cooled) from the system?
CO + H2O ⟷ CO2 + H2 ΔH = +41.4 kJ
\
Both reactants and products would be produced.
Shift right.
Shift left.
This equation does not represent an equilibrium system.
Neither reactant nor products would be produced.
CO + H2O ⟷ CO2 + H2 ΔH = +41.4 kJ
\
Both reactants and products would be produced.
Shift right.
Shift left.
This equation does not represent an equilibrium system.
Neither reactant nor products would be produced.
Shift left
19
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Use LeChatlier’s Principle to determine which variable(s) will best favor the products in the following equilibrium.
N2O4(g) ⟷ 2NO2(g) ΔH=+57.2 kJ/mole
\
Decrease in temperature and increase in total pressure.
Increase in temperature and decrease in total pressure.
Decrease in temperature and decrease in total pressure.
Increase in temperature and increase in total pressure.
Temperature and total pressure have no effect on this equilibrium.
N2O4(g) ⟷ 2NO2(g) ΔH=+57.2 kJ/mole
\
Decrease in temperature and increase in total pressure.
Increase in temperature and decrease in total pressure.
Decrease in temperature and decrease in total pressure.
Increase in temperature and increase in total pressure.
Temperature and total pressure have no effect on this equilibrium.
Increase in temperature and decrease in total pressure.
20
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CHAPTER 17 ACID-BASE REACTIONS
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Identify the base and conjugate acid.
Na2HPO4 + H2CO3 ⟷NaH2PO4 + NaHCO3
H2CO3 is the acid, Na2HPO4 is the conjugate base.
H2CO3 is the acid, NaHCO3 is the conjugate base.
H2CO3 is the acid, NaH2PO4 is the conjugate base.
Na2HPO4 is the acid, H2CO3 is the conjugate base.
Na2HPO4 is the base, NaH2PO4 is the conjugate acid.
Na2HPO4 + H2CO3 ⟷NaH2PO4 + NaHCO3
H2CO3 is the acid, Na2HPO4 is the conjugate base.
H2CO3 is the acid, NaHCO3 is the conjugate base.
H2CO3 is the acid, NaH2PO4 is the conjugate base.
Na2HPO4 is the acid, H2CO3 is the conjugate base.
Na2HPO4 is the base, NaH2PO4 is the conjugate acid.
Na2HPO4 is the base, NaH2PO4 is the conjugate acid.
22
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1\.60 mL of a suspension of 320.0 mg/5.00 mL aluminum hydroxide is added to 2.80 mL of hydrochloric acid. What is the molarity of the hydrochloric acid?
\
1\.41 M
0\.549 M
0\.711 M
0\.469 M
0\.156 M
\
1\.41 M
0\.549 M
0\.711 M
0\.469 M
0\.156 M
1\.41 M
23
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The basis for the pH scale is explained by:
\
The intermolecular forces of water.
The molecular polarity of water.
The molecular structure of water.
The specific heat capacity of water.
The autoionization of water.
\
The intermolecular forces of water.
The molecular polarity of water.
The molecular structure of water.
The specific heat capacity of water.
The autoionization of water.
The autoionization of water.
24
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Which of the following results in the formation of the hydronium ion?
\
Base reacting with a conjugate acid.
Acid reacting with a conjugate base.
Acid-base reaction.
Base dissociation.
Acid dissociation.
\
Base reacting with a conjugate acid.
Acid reacting with a conjugate base.
Acid-base reaction.
Base dissociation.
Acid dissociation.
Acid dissociation.
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Which of the following do not have acidic properties?
Proteins
Hydrolyzed fat
DNA
RNA
Carbohydrates
Proteins
Hydrolyzed fat
DNA
RNA
Carbohydrates
Carbohydrates
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Calculate the pH for a 0.348 M HNO3 solution.
\-0.458
\-5.85
5\.85
0\.458
An HCl solution is pH 7 (neutral), because no H+1 are present.
\-0.458
\-5.85
5\.85
0\.458
An HCl solution is pH 7 (neutral), because no H+1 are present.
0\.458
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What chemical species are present after the dissociation of chromic acid has reached equilibrium?
\
Chromic acid, hydrogen chromate ion, hydrogen ion.
Chromic acid, chromate ion, hydrogen ion.
Chromic acid, hydrogen chromate ion, chromate ion, hydrogen ion.
Hydrogen chromate ion, chromate ion, hydrogen ion.
Chromate ion, hydrogen ion.
\
Chromic acid, hydrogen chromate ion, hydrogen ion.
Chromic acid, chromate ion, hydrogen ion.
Chromic acid, hydrogen chromate ion, chromate ion, hydrogen ion.
Hydrogen chromate ion, chromate ion, hydrogen ion.
Chromate ion, hydrogen ion.
Chromic acid, hydrogen chromate ion, chromate ion, hydrogen ion.
28
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Identify the Bronsted-Lowry acid and base?
K2Cr2O7 + H2SO4 ⟷ H2Cr2O7 +K2SO4
\
H2Cr2O7 is the acid, K2SO4 is the base.
\
K2Cr2O7 is the base, H2SO4 is the acid.
\
There is no Bronsted-Lowry acid or base in this equation.
K2SO4 is the acid, H2Cr2O7 is the base.
K2Cr2O7 is the acid, H2SO4 is the base.
K2Cr2O7 + H2SO4 ⟷ H2Cr2O7 +K2SO4
\
H2Cr2O7 is the acid, K2SO4 is the base.
\
K2Cr2O7 is the base, H2SO4 is the acid.
\
There is no Bronsted-Lowry acid or base in this equation.
K2SO4 is the acid, H2Cr2O7 is the base.
K2Cr2O7 is the acid, H2SO4 is the base.
K2Cr2O7 is the base, H2SO4 is the acid.
29
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The condition of blood alkalosis is a result of:
Blood pH above 7.4 and a hydrogen ion concentration higher than normal.
Blood pH below 7.4 and a hydrogen ion concentration lower than normal.
Blood pH below 7.4 and a hydrogen ion concentration higher than normal.
Blood pH below 7.0 and a hydrogen ion concentration lower than normal.
Blood pH above 7.4 and a hydrogen ion concentration lower than normal.
Blood pH above 7.4 and a hydrogen ion concentration higher than normal.
Blood pH below 7.4 and a hydrogen ion concentration lower than normal.
Blood pH below 7.4 and a hydrogen ion concentration higher than normal.
Blood pH below 7.0 and a hydrogen ion concentration lower than normal.
Blood pH above 7.4 and a hydrogen ion concentration lower than normal.
Blood pH above 7.4 and a hydrogen ion concentration lower than normal.
30
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155 mL of hydrochloric acid solution is used to react 4.30 g magnesium hydroxide. Calculate the molarity of the hydrochloric solution.
\
0\.672 M
0\.476 M
1\.34 M
0\.951 M
1\.05 M
\
0\.672 M
0\.476 M
1\.34 M
0\.951 M
1\.05 M
0\.951 M
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Which of the following is the definition of a base?
An Arrhenius base is a substance capable of producing H+1; A Bronsted-Lowry base is a substance accepting a hydrogen ion.
An Arrhenius base is a substance capable of producing H+1; A Bronsted-Lowry base is a substance donating a hydrogen ion.
An Arrhenius base is a substance capable of donating H+1; A Bronsted-Lowry base is a substance capable of producing a hydrogen ion.
An Arrhenius base is a substance capable of producing OH-1; A Bronsted-Lowry base is a substance donating a hydrogen ion.
An Arrhenius base is a substance capable of producing OH-1; A Bronsted-Lowry base is a substance accepting a hydrogen ion.
An Arrhenius base is a substance capable of producing H+1; A Bronsted-Lowry base is a substance accepting a hydrogen ion.
An Arrhenius base is a substance capable of producing H+1; A Bronsted-Lowry base is a substance donating a hydrogen ion.
An Arrhenius base is a substance capable of donating H+1; A Bronsted-Lowry base is a substance capable of producing a hydrogen ion.
An Arrhenius base is a substance capable of producing OH-1; A Bronsted-Lowry base is a substance donating a hydrogen ion.
An Arrhenius base is a substance capable of producing OH-1; A Bronsted-Lowry base is a substance accepting a hydrogen ion.
An Arrhenius base is a substance capable of producing OH-1; A Bronsted-Lowry base is a substance accepting a hydrogen ion.
32
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dentify the acid and the conjugate acid in the following chemical equation:
PO4-3(aq) + HC2O4-1(aq) ⟷ HPO4-2 (aq) + C2O4-2(aq)
The acid is PO4-3(aq), the conjugate acid is C2O4-2(aq).
The acid is HC2O4-1(aq), but there is no conjugate acid.
The acid is HC2O4-1(aq), the conjugate acid is C2O4-2(aq).
The acid is HC2O4-1(aq), the conjugate acid is HPO4-2(aq).
The acid is PO4-3(aq), the conjugate acid is HPO4-2 (aq).
PO4-3(aq) + HC2O4-1(aq) ⟷ HPO4-2 (aq) + C2O4-2(aq)
The acid is PO4-3(aq), the conjugate acid is C2O4-2(aq).
The acid is HC2O4-1(aq), but there is no conjugate acid.
The acid is HC2O4-1(aq), the conjugate acid is C2O4-2(aq).
The acid is HC2O4-1(aq), the conjugate acid is HPO4-2(aq).
The acid is PO4-3(aq), the conjugate acid is HPO4-2 (aq).
The acid is HC2O4-1(aq), the conjugate acid is HPO4-2(aq).
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Which of the following is true about the pH scale?
\
A decrease from pH 2 to pH 1 is a 10-fold increase in hydrogen ion concentration.
A decrease from pH 2 to pH 1 is a 2-fold increase in hydrogen ion concentration.
A decrease from pH 2 to pH 1 is a 2-fold decrease in hydrogen ion concentration.
A decrease from pH 2 to pH 1 is an 8-fold increase in hydrogen ion concentration.
A decrease from pH 2 to pH 1 is a 4-fold increase in hydrogen ion concentration.
\
A decrease from pH 2 to pH 1 is a 10-fold increase in hydrogen ion concentration.
A decrease from pH 2 to pH 1 is a 2-fold increase in hydrogen ion concentration.
A decrease from pH 2 to pH 1 is a 2-fold decrease in hydrogen ion concentration.
A decrease from pH 2 to pH 1 is an 8-fold increase in hydrogen ion concentration.
A decrease from pH 2 to pH 1 is a 4-fold increase in hydrogen ion concentration.
A decrease from pH 2 to pH 1 is a 10-fold increase in hydrogen ion concentration.
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Which of the following is a weak acid?
\
HF
HI
HClO4
HCl
HNO3
\
HF
HI
HClO4
HCl
HNO3
HF
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Calculate the pH of a solution with an H+1 concentration of 2.90 x10-12and identify the solution as acid, base or neutral.
pH = 26.6, neutral
pH = 11.5, acid
pH = 11.5, base
pH = 26.6, base
pH = 26.6, acid
pH = 26.6, neutral
pH = 11.5, acid
pH = 11.5, base
pH = 26.6, base
pH = 26.6, acid
pH = 11.5, base
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Which of the following reactants/products are present when sulfuric acid is mixed with water?
H2SO4(aq) ⟶ H+1(aq) + HSO4-1(aq)
HSO4-1(aq) ⟷ H+1(aq) + SO4-2(aq)
\
H2SO4(aq), H+1(aq), HSO4-1(aq)
H2SO4(aq), HSO4-1(aq), SO4-2(aq)
H+1(aq), SO4-2(aq)
\
HSO4-1(aq), H+1(aq), SO4-2(aq)
H2SO4(aq), H+1(aq), SO4-2(aq)
H2SO4(aq) ⟶ H+1(aq) + HSO4-1(aq)
HSO4-1(aq) ⟷ H+1(aq) + SO4-2(aq)
\
H2SO4(aq), H+1(aq), HSO4-1(aq)
H2SO4(aq), HSO4-1(aq), SO4-2(aq)
H+1(aq), SO4-2(aq)
\
HSO4-1(aq), H+1(aq), SO4-2(aq)
H2SO4(aq), H+1(aq), SO4-2(aq)
HSO4-1(aq), H+1(aq), SO4-2(aq)
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Aluminum hydroxide reacts with stomach acid (hydrochloric acid). Calculate the molarity of the stomach acid if 0.545 g aluminum hydroxide is used to react 39.0 mL of stomach acid using the following balanced equation.
Al(OH)3 + 3HCl ⟶ AlCl3 + 3H2O
0\.0597 M
0\.179 M
0\.553 M
0\.000818 M
0\.537 M
Al(OH)3 + 3HCl ⟶ AlCl3 + 3H2O
0\.0597 M
0\.179 M
0\.553 M
0\.000818 M
0\.537 M
0\.537 M
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Write the dissociation equation for ammonium hydroxide in solution?
NH4OH(aq) ⟶ NH4(aq) + OH(aq)
\
NH4OH(aq) ⟷ NH4+1(aq) + OH-1(aq)
Ammonium hydroxide does not dissociate.
NH4OH(aq) ⟷ NH4(aq) + OH(aq)
NH4OH(aq) ⟶ NH4+1(aq) + OH-1(aq)
NH4OH(aq) ⟶ NH4(aq) + OH(aq)
\
NH4OH(aq) ⟷ NH4+1(aq) + OH-1(aq)
Ammonium hydroxide does not dissociate.
NH4OH(aq) ⟷ NH4(aq) + OH(aq)
NH4OH(aq) ⟶ NH4+1(aq) + OH-1(aq)
NH4OH(aq) ⟷ NH4+1(aq) + OH-1(aq)
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Which of the following characteristics applies to water?
Water is neutral, but also amphoteric, it acts as neither acid or base during chemical reactions.
Water is basic.
Water is acidic.
Water is neutral, but also amphoteric, it acts as either acid or base during chemical reactions.
Water is neutral.
Water is neutral, but also amphoteric, it acts as neither acid or base during chemical reactions.
Water is basic.
Water is acidic.
Water is neutral, but also amphoteric, it acts as either acid or base during chemical reactions.
Water is neutral.
Water is neutral, but also amphoteric, it acts as either acid or base during chemical reactions.
40
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Which of the following is true about the following equation?
NH3(g) + H2O(l) ⟷NH4+1(aq) + OH-1(aq)
\
Ammonia is a Brontsted-Lowry base because it accepts a hydrogen ion.
Ammonia is an Arrhenius base because it accepts a hydrogen ion.
Ammonia is a Brontsted-Lowry base because it donates a hydrogen ion.
Ammonia is an Arrhenius base because it produces a hydroxide ion.
NH3(g) + H2O(l) ⟷NH4+1(aq) + OH-1(aq)
\
Ammonia is a Brontsted-Lowry base because it accepts a hydrogen ion.
Ammonia is an Arrhenius base because it accepts a hydrogen ion.
Ammonia is a Brontsted-Lowry base because it donates a hydrogen ion.
Ammonia is an Arrhenius base because it produces a hydroxide ion.
Ammonia is a Brontsted-Lowry base because it accepts a hydrogen ion.
41
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CHAPTER 16: SOLUTIONS
42
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Calculate the mass (in kg) of solvent required to make 1.20 kg of a 2.20% sodium acetate solution by mass.
0\.0183 kg
1\.17 kg
0\.545 kg
0\.655 kg
0\.0264 kg
0\.0183 kg
1\.17 kg
0\.545 kg
0\.655 kg
0\.0264 kg
1\.17 kg
43
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Calculate the mass (in grams) of solute for 445 mL of a 3.80% mass by volume solution of sodium bicarbonate.
328 kg
0\.854 g
428 g
117 g
16\.9 g
328 kg
0\.854 g
428 g
117 g
16\.9 g
16\.9 g
44
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How many L of solute are required to make 5.70 L of a 70.0% by volume isopropyl alcohol solution?
5\.58 L
0\.0814 L
0\.123 L
1\.71 L
3\.99 L
5\.58 L
0\.0814 L
0\.123 L
1\.71 L
3\.99 L
3\.99 L
45
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Calculate the molarity of a solution prepared by adding 17.3 g sodium sulfate to a total volume of 864 mL.
0\.168 M
0\.0499 M
0\.141 M
7\.09 M
2\.84 M
0\.168 M
0\.0499 M
0\.141 M
7\.09 M
2\.84 M
0\.141 M
46
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Calculate the concentration for 84.0 mL of a 12.0% by mass HCl solution diluted with 285 mL of water.
\
9\.27%
3\.54%
5\.01%
0\.526%
2\.73%
\
9\.27%
3\.54%
5\.01%
0\.526%
2\.73%
2\.73%
47
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One system consists of a permeable membrane with an intracellular concentration greater than the extracellular concentration. A second system is a semi-permeable membrane with equal intracellular and extracellular concentration. Describe the solution type for each system.
\
The permeable membrane is hypertonic, the semi-permeable membrane is isotonic.
\
The permeable membrane is hypotonic, the semi-permeable membrane is isotonic.
The permeable membrane is isotonic, the semi-permeable membrane is hypertonic.
\
Both systems are isotonic.
The permeable membrane is isotonic, the semi-permeable membrane is hypotonic.
\
The permeable membrane is hypertonic, the semi-permeable membrane is isotonic.
\
The permeable membrane is hypotonic, the semi-permeable membrane is isotonic.
The permeable membrane is isotonic, the semi-permeable membrane is hypertonic.
\
Both systems are isotonic.
The permeable membrane is isotonic, the semi-permeable membrane is hypotonic.
Both systems are isotonic.
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How is a solution freezing point and boiling point affected by addition of a dissolved solute?
The freezing point and boiling point are independent of dissolved solute concentratio.
The freezing point and boiling point are decreased.
The freezing point and boiling point are increased.
The freezing point decreases, the boiling point increases.
The freezing point increases, the boiling point decreases.
The freezing point and boiling point are independent of dissolved solute concentratio.
The freezing point and boiling point are decreased.
The freezing point and boiling point are increased.
The freezing point decreases, the boiling point increases.
The freezing point increases, the boiling point decreases.
The freezing point decreases, the boiling point increases.
49
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Which of the following affect the internal osmotic pressure of a system, such as a cell?
Osmotic pressure is independent of volume changes.
Osmotic pressure decreases with a decrease in volume and decreases with an increase in concentration.
Osmotic pressure increases with a decrease in volume and decreases with an increase in concentration.
Osmotic pressure increases with a decrease in volume and increases with an increase in concentration.
Osmotic pressure is independent of volume changes.
Osmotic pressure decreases with a decrease in volume and decreases with an increase in concentration.
Osmotic pressure increases with a decrease in volume and decreases with an increase in concentration.
Osmotic pressure increases with a decrease in volume and increases with an increase in concentration.
Osmotic pressure increases with a decrease in volume and increases with an increase in concentration.
50
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Calculate the volume (in mL) per dose for 275. mg/mL amoxicillin to deliver two doses per day at 40.0 mg/(kg⋅day) for a 22.0 pound patient. 2.20 pounds = 1 kg.
0\.275 mL/dose
13\.8 mL/dose
33\.3 mL/dose
3\.64 mL/dose
0\.727 mL/dose
0\.275 mL/dose
13\.8 mL/dose
33\.3 mL/dose
3\.64 mL/dose
0\.727 mL/dose
0\.727 mL/dose
51
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A 110.0 pound patient is to receive Heparin by IV with an infusion rate of 29.0 Units/(kg⋅hour). Heparin is supplied at 25,000.0 Units in 250.0 mL. How many mL per hour should the IV pump be set for this infusion? 2.20 pounds = 1 kg.
58\.0 mL/hour
70\.2 mL/hour
31\.9 mL/hour
\
14\.5 mL/hour
0\.0690 mL/hour
58\.0 mL/hour
70\.2 mL/hour
31\.9 mL/hour
\
14\.5 mL/hour
0\.0690 mL/hour
14\.5 mL/hour
52
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How many grams of sucrose are needed to prepare 500.0 g of a solution that is 10.00 % by mass sucrose?
500\.0 g
0\.5000 g
5000\. g
50\.00 g
450\.0 g
500\.0 g
0\.5000 g
5000\. g
50\.00 g
450\.0 g
50\.00 g
53
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A solution was prepared by mixing 10.00 g of NaCl in 100.0 g of water. What is the percent concentration of the solution?
1\.000%
0\.1000%
10\.00%
11\.11%
9\.091%
1\.000%
0\.1000%
10\.00%
11\.11%
9\.091%
9\.091%
54
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Calculate the grams of solute in 45.0 mL of a 12.0 % (w/v) boric acid solution?
0\.267 g
5\.40 g
39\.6 g
540\. g
3\.75 g
0\.267 g
5\.40 g
39\.6 g
540\. g
3\.75 g
5\.40 g
55
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A 975 mL of a 65.0 % (v/v) isopropyl alcohol solution contains how many mL of isopropyl alcohol?
0\.150 mL
634 mL
341 mL
0\.0667 mL
1\.50x103 mL
0\.150 mL
634 mL
341 mL
0\.0667 mL
1\.50x103 mL
634 mL
56
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Calculate the number of grams of solute required to prepare 200. mL of a 0.400 M acetic acid (HC2H3O2) solution.
\
4\.80 g
24\.0 g
120\. g
1\.33 g
80\.0 g
\
4\.80 g
24\.0 g
120\. g
1\.33 g
80\.0 g
4\.80 g
57
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What is the molarity of 500.0 mL of a solution containing 57.0 g of HNO3?
1\.81 M
0\.452 M
28\.5 M
7\.18 M
0\.114 M
1\.81 M
0\.452 M
28\.5 M
7\.18 M
0\.114 M
1\.81 M
58
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85\.0 g of solute is added to 450.0 g of solvent, what is the percent concentration of the solution?
5\.29%
18\.9%
6\.29%
23\.3%
15\.9%
5\.29%
18\.9%
6\.29%
23\.3%
15\.9%
15\.9%
59
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If 45.0 mL of solvent is added to 85.0 mL of an 80.0% solution, what would the new concentration be?
80\.0%
1\.63%
90\.3%
61\.5%
\
52\.3%
80\.0%
1\.63%
90\.3%
61\.5%
\
52\.3%
52\.3%
60
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A solution has a higher intracellular concentration, what type of solution is it?
Unsaturated
Hypertonic
Hypotonic
Saturated
Isotonic
Unsaturated
Hypertonic
Hypotonic
Saturated
Isotonic
Hypotonic
61
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Which of the following is required for osmotic pressure?
Concentration differential of ions across a porous membrane.
Concentration differential across a membrane.
Concentration differential across a porous membrane.
Concentration differential across a semi-permeable membrane.
Concentration differential across a permeable membrane.
Concentration differential of ions across a porous membrane.
Concentration differential across a membrane.
Concentration differential across a porous membrane.
Concentration differential across a semi-permeable membrane.
Concentration differential across a permeable membrane.
Concentration differential across a semi-permeable membrane.
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CHAPTER 15
63
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Identify the intermolecular force involved with the mixing of nitrogen and water.
Ion-induced dipole intermolecular forces
Ion-dipole intermolecular forces
Hydrogen bonding
Dispersion forces
Dipole-dipole Intermolecular forces
\
Dipole-induced dipole intermolecular forces
Ion-induced dipole intermolecular forces
Ion-dipole intermolecular forces
Hydrogen bonding
Dispersion forces
Dipole-dipole Intermolecular forces
\
Dipole-induced dipole intermolecular forces
Dipole-induced dipole intermolecular forces
64
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Identify the intermolecular force involved with the mixing of sulfur trioxide and water.
Ion-induced dipole intermolecular forces
Ion-dipole intermolecular forces
\
Dipole-induced dipole intermolecular forces
Hydrogen bonding
Dipole-dipole Intermolecular forces
Dispersion forces
Ion-induced dipole intermolecular forces
Ion-dipole intermolecular forces
\
Dipole-induced dipole intermolecular forces
Hydrogen bonding
Dipole-dipole Intermolecular forces
Dispersion forces
Dipole-induced dipole intermolecular forces
\
\
65
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Calculate the total energy in kJ required to change the temperature of 786 g water from 96.0 oC to -111 oC.
__Water Physical Property Data Table__
Heat capacity for ice is 0.00206 kJ/(g oC)
Heat capacity for liquid water is 0.00418 kJ/(g oC)
Heat capacity for steam (water vapor) is 0.00200 kJ/(g oC)
Heat of fusion (ΔHfusion) for water in the liquid state is 0.333 kJ/g
Heat of vaporization (ΔHvap) for water in the gaseous state is 2.26 kJ/g
\
\
\+674 kJ
\+757 kJ
\+335 kJ
\
\-757 kJ
\-335 kJ
\
__Water Physical Property Data Table__
Heat capacity for ice is 0.00206 kJ/(g oC)
Heat capacity for liquid water is 0.00418 kJ/(g oC)
Heat capacity for steam (water vapor) is 0.00200 kJ/(g oC)
Heat of fusion (ΔHfusion) for water in the liquid state is 0.333 kJ/g
Heat of vaporization (ΔHvap) for water in the gaseous state is 2.26 kJ/g
\
\
\+674 kJ
\+757 kJ
\+335 kJ
\
\-757 kJ
\-335 kJ
\
\-757 kJ
66
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Calculate the total energy in kJ required to change the temperature of 199 g water from 19.0 oC to 78.0 oC.
__Water Physical Property Data Table__
Heat capacity for ice is 0.00206 kJ/(g oC)
Heat capacity for liquid water is 0.00418 kJ/(g oC)
Heat capacity for steam (water vapor) is 0.00200 kJ/(g oC)
Heat of fusion (ΔHfusion) for water in the liquid state is 0.333 kJ/g
Heat of vaporization (ΔHvap) for water in the gaseous state is 2.26 kJ/g
\
\+49.1 kJ
\+45.9 kJ
\+24.2 kJ
23\.5 kJ
\+3910 kJ
__Water Physical Property Data Table__
Heat capacity for ice is 0.00206 kJ/(g oC)
Heat capacity for liquid water is 0.00418 kJ/(g oC)
Heat capacity for steam (water vapor) is 0.00200 kJ/(g oC)
Heat of fusion (ΔHfusion) for water in the liquid state is 0.333 kJ/g
Heat of vaporization (ΔHvap) for water in the gaseous state is 2.26 kJ/g
\
\+49.1 kJ
\+45.9 kJ
\+24.2 kJ
23\.5 kJ
\+3910 kJ
\+49.1 kJ
67
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The boiling point of water assuming constant external pressure is determined by:
Ionic bonding
Covalent bonding
Hydrogen bonding
Dispersion forces
Polar covalent bonding
Ionic bonding
Covalent bonding
Hydrogen bonding
Dispersion forces
Polar covalent bonding
Hydrogen bonding
68
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An aqueous chemical reaction produces hydrogen gas with a total pressure of 547.0 torr at 17.5 oC in a closed container. What is the partial pressure of the hydrogen gas if the water vapor pressure is 15.0 torr at 17.5 oC and external atmospheric pressure is 760.0 torr?
Mg(s) + 2HCl(aq) ⟶H2(g) + MgCl2(aq)
\
532\.0 torr
213\.0 torr
745\.0 torr
562\.0 torr
775\.0 torr
Mg(s) + 2HCl(aq) ⟶H2(g) + MgCl2(aq)
\
532\.0 torr
213\.0 torr
745\.0 torr
562\.0 torr
775\.0 torr
532\.0 torr
69
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which of the following explains the transport of oxygen in the circulatory system?
Oxygen is dissolved in the blood plasma and carried by water with hydrogen bonding.
Oxygen is transported to the red blood cells and carried by hemoglobin protein with hydrogen bonding.
Oxygen is dissolved in the blood plasma and carried by water with dipole-induced dipole forces.
Oxygen is transported to the red blood cells and carried by hemoglobin protein with ion-dipole forces.
Oxygen is transported to the red blood cells and carried by hemoglobin protein with ion-induced dipole forces.
Oxygen is dissolved in the blood plasma and carried by water with hydrogen bonding.
Oxygen is transported to the red blood cells and carried by hemoglobin protein with hydrogen bonding.
Oxygen is dissolved in the blood plasma and carried by water with dipole-induced dipole forces.
Oxygen is transported to the red blood cells and carried by hemoglobin protein with ion-dipole forces.
Oxygen is transported to the red blood cells and carried by hemoglobin protein with ion-induced dipole forces.
Oxygen is transported to the red blood cells and carried by hemoglobin protein with ion-induced dipole forces.
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Which of the following is true about water?
Ice floats on liquid water because the three dimensional structure of water in the liquid state is less dense than the solid state.
Ice sinks in liquid water because the three dimensional structure of water in the liquid state is more dense than the solid state.
Ice floats on liquid water because the three dimensional structure of water in the liquid state is more dense than the solid state.
The density of water does not change between the solid and liquid states.
Ice sinks in liquid water because the three dimensional structure of water in the liquid state is less dense than the solid state.
Ice floats on liquid water because the three dimensional structure of water in the liquid state is less dense than the solid state.
Ice sinks in liquid water because the three dimensional structure of water in the liquid state is more dense than the solid state.
Ice floats on liquid water because the three dimensional structure of water in the liquid state is more dense than the solid state.
The density of water does not change between the solid and liquid states.
Ice sinks in liquid water because the three dimensional structure of water in the liquid state is less dense than the solid state.
Ice floats on liquid water because the three dimensional structure of water in the liquid state is more dense than the solid state.
71
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Using the heat versus temperature diagram determine which of the following is true.
An increase in heat results in an increase in temperature except at the boiling point because of a change in intermolecular forces.
An increase in heat results in an increase in temperature due to changes in intermolecular forces except the boiling point and freezing point.
An increase in heat results in an increase in temperature except at the freezing point because of a change in intermolecular forces.
\
An increase in heat results in an increase in temperature except the freezing point and boiling point do not change temperature because of changes in intermolecular forces.
An increase in heat results in an increase in temperature because of a change in intermolecular forces.
An increase in heat results in an increase in temperature except at the boiling point because of a change in intermolecular forces.
An increase in heat results in an increase in temperature due to changes in intermolecular forces except the boiling point and freezing point.
An increase in heat results in an increase in temperature except at the freezing point because of a change in intermolecular forces.
\
An increase in heat results in an increase in temperature except the freezing point and boiling point do not change temperature because of changes in intermolecular forces.
An increase in heat results in an increase in temperature because of a change in intermolecular forces.
An increase in heat results in an increase in temperature except the freezing point and boiling point do not change temperature because of changes in intermolecular forces.
72
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What characteristic of substances does specific heat capacity and heat of vaporization measure?
Specific heat capacity and heat of vaporization measure the amount of energy released or absorbed during a chemical reaction.
Specific heat capacity measures the amount of heat energy required to break or form intermolecular forces to change state while heat of vaporization is the amount of heat energy retained.
Specific heat capacity measures the amount of heat energy retained as intermolecular forces, while heat of vaporization is the amount of energy required to change state.
Specific heat capacity measures the amount of heat energy retained, while heat of vaporization is the amount of energy required to break or form intermolecular forces to change state.
Specific heat capacity measures the amount of heat energy required to break intermolecular forces to change state while heat of vaporization is the amount of heat energy retained as intermolecular forces to change state.
Specific heat capacity and heat of vaporization measure the amount of energy released or absorbed during a chemical reaction.
Specific heat capacity measures the amount of heat energy required to break or form intermolecular forces to change state while heat of vaporization is the amount of heat energy retained.
Specific heat capacity measures the amount of heat energy retained as intermolecular forces, while heat of vaporization is the amount of energy required to change state.
Specific heat capacity measures the amount of heat energy retained, while heat of vaporization is the amount of energy required to break or form intermolecular forces to change state.
Specific heat capacity measures the amount of heat energy required to break intermolecular forces to change state while heat of vaporization is the amount of heat energy retained as intermolecular forces to change state.
Specific heat capacity measures the amount of heat energy retained, while heat of vaporization is the amount of energy required to break or form intermolecular forces to change state.
73
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The physical properties of water can be explained by:
Metallic bonding
\
Hydrogen bonding
Ion-Dipole intermolecular forces
Dispersion forces
Dipole-Dipole Intermolecular forces
Ionic bonding
Covalent bonding
Dipole-induced dipole intermolecular forces
Ion-induced dipole intermolecular forces
Polar covalent bonding
Metallic bonding
\
Hydrogen bonding
Ion-Dipole intermolecular forces
Dispersion forces
Dipole-Dipole Intermolecular forces
Ionic bonding
Covalent bonding
Dipole-induced dipole intermolecular forces
Ion-induced dipole intermolecular forces
Polar covalent bonding
Hydrogen bonding
74
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Identify the primary intermolecular force involved in the oxygenation of water.
Hydrogen bonding
Dipole-Dipole Intermolecular forces
Ion-Dipole intermolecular forces
Dispersion forces
\
Dipole-induced dipole intermolecular forces
Ion-induced dipole intermolecular forces
Hydrogen bonding
Dipole-Dipole Intermolecular forces
Ion-Dipole intermolecular forces
Dispersion forces
\
Dipole-induced dipole intermolecular forces
Ion-induced dipole intermolecular forces
Dipole-induced dipole intermolecular forces
75
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Calculate the heat required in units of kJ to raise the temperature of 1.20 kg of water from 14.0 oC to 55.0 oC? The specific heat capacity for water is 4.184 J/(g·oC).
\
\+206 kJ
\+0.206 kJ
\-206 kJ
11\.8 kJ
\-0.206 kJ
\
\+206 kJ
\+0.206 kJ
\-206 kJ
11\.8 kJ
\-0.206 kJ
\+206 kJ
76
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The physical property for viscosity of nonpolar hydrocarbons is based on:
Increased molecule length results in decreased viscosity due to dipole-induced dipole interactions.
Increased molecule length results in greater viscosity due to hydrogen bonding.
Increased molecule length results in decreased viscosity due to hydrogen bonding.
\
Increased molecule length results in greater viscosity due to dispersion forces.
Increased molecule length results in decreased viscosity due to dispersion forces.
Increased molecule length results in decreased viscosity due to dipole-induced dipole interactions.
Increased molecule length results in greater viscosity due to hydrogen bonding.
Increased molecule length results in decreased viscosity due to hydrogen bonding.
\
Increased molecule length results in greater viscosity due to dispersion forces.
Increased molecule length results in decreased viscosity due to dispersion forces.
Increased molecule length results in greater viscosity due to dispersion forces.
77
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Calculate the energy required (in units of kJ) to heat 12.00 g water from 22.00 oC to 115.0 oC? Specific heat capacity for liquid water is 4.184 J/(g·oC), the heat capacity for water vapor is 2.000 J/(g·oC). The heat of vaporization for water in the gaseous state is 2260.0 J/g.
2\.23 kJ
31\.0 kJ
\
31\.4 kJ
5\.75 kJ
4\.28 kJ
2\.23 kJ
31\.0 kJ
\
31\.4 kJ
5\.75 kJ
4\.28 kJ
31\.4 kJ
78
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DNA structure is composed of the following:
Covalent bonding between nucleotides and ion-dipole forces along the backbone.
Covalent bonding between nucleotides and hydrogen bonding along the backbone.
Polar covalent bonding between the nucleotides and ionic bonding along the backbone.
\
Hydrogen bonding between nucleotides and covalent bonding along the backbone.
Covalent bonding between nucleotides and ion-dipole forces along the backbone.
Covalent bonding between nucleotides and hydrogen bonding along the backbone.
Polar covalent bonding between the nucleotides and ionic bonding along the backbone.
\
Hydrogen bonding between nucleotides and covalent bonding along the backbone.
Hydrogen bonding between nucleotides and covalent bonding along the backbone.
79
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Calculate the pressure of chlorine gas collected over water with a total vapor pressure of 1.140 atm at 20.0 oC? The water vapor pressure at 20.0 oC is 17.5 mm Hg.
\
1\.12 atm
16\.4 atm
1\.16 atm
18\.6 atm
42\.3 atm
\
1\.12 atm
16\.4 atm
1\.16 atm
18\.6 atm
42\.3 atm
1\.12 atm
80
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Toxicity of carbon monoxide can be explained by which of the following?
Dispersion forces
Ion-induced dipole intermolecular force
**You Answered**
Polar covalent bonding
\
Ion-dipole intermolecular forces
Ionic bonding
Dipole-dipole intermolecular force
Covalent bonding
Hydrogen bonding
Dipole-induced dipole intermolecular force
Metallic bonding
Dispersion forces
Ion-induced dipole intermolecular force
**You Answered**
Polar covalent bonding
\
Ion-dipole intermolecular forces
Ionic bonding
Dipole-dipole intermolecular force
Covalent bonding
Hydrogen bonding
Dipole-induced dipole intermolecular force
Metallic bonding
Ion-dipole intermolecular forces
81
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A measured heat value is -1.18 J resulting in a temperature change, what does this mean?
1\.18 J of energy absorbed to increase kinetic energy of the system.
1\.18 J of energy released to decrease kinetic energy of the system.
1\.18 J of energy is released from the system by gain of kinetic energy and change in intermolecular forces.
1\.18 J of energy is released from the system by loss of kinetic energy and change in intermolecular forces.
1\.18 J of energy released from the system to change intermolecular forces.
1\.18 J of energy absorbed to increase kinetic energy of the system.
1\.18 J of energy released to decrease kinetic energy of the system.
1\.18 J of energy is released from the system by gain of kinetic energy and change in intermolecular forces.
1\.18 J of energy is released from the system by loss of kinetic energy and change in intermolecular forces.
1\.18 J of energy released from the system to change intermolecular forces.
1\.18 J of energy released to decrease kinetic energy of the system.
82
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Calculate the heat (in kJ) for a 2.80 kg system changing temperature from 85.0 oC to 10.0 oC? The specific heat capacity is 0.386 J/(g·oC).
\+ 81.1 kJ
\-81.1 kJ
\-8.11 x104 kJ
\+544 kJ
\+8.11 x104 kJ
\+ 81.1 kJ
\-81.1 kJ
\-8.11 x104 kJ
\+544 kJ
\+8.11 x104 kJ
\-81.1 kJ
83
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CHAPTER 14
84
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Use the following equation to calculate the grams of CaH2 to generate 29.2 L of hydrogen gas at STP.
CaH2(s) + 2H2O(l) → Ca(OH)2(s) + 2H2(g)
\
110\. g
305 g
27\.4 g
54\.9 g
31\.1 g
CaH2(s) + 2H2O(l) → Ca(OH)2(s) + 2H2(g)
\
110\. g
305 g
27\.4 g
54\.9 g
31\.1 g
27\.4 g
\
\
85
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CHAPTER 13
86
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Which of the following best summarizes VSEPR theory?
Electrons maximize distance to maximize repulsion.
Electrons maximize distance to minimize repulsion.
Electrons minimize distance to minimize repulsion.
Electrons minimize distance to maximize repulsion.
Electron distance is averaged due to repulsion.
Electrons maximize distance to maximize repulsion.
Electrons maximize distance to minimize repulsion.
Electrons minimize distance to minimize repulsion.
Electrons minimize distance to maximize repulsion.
Electron distance is averaged due to repulsion.
Electrons maximize distance to maximize repulsion.
87
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How many bonding electron pair(s) and lone electron pair(s) are located on the central nitrogen atom in ammonia?
Three bonding pair, zero lone pair
One bonding pair, three lone pair
Four bonding pair, zero lone pair
Three bonding pair, one lone pair
Two bonding pair, two lone pair
Three bonding pair, zero lone pair
One bonding pair, three lone pair
Four bonding pair, zero lone pair
Three bonding pair, one lone pair
Two bonding pair, two lone pair
Three bonding pair, one lone pair
88
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Determine the molecular geometry and molecular polarity for the molecule SiO2.
linear nonpolar
89
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Determine the molecular geometry and molecular polarity for chlorate.
Trigonal pyramidal ionic
90
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What is the molecular geometry and molecular polarity of CCl2F2?
Tetrahedral nonpolar
91
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Determine the molecular geometry and molecular polarity for periodate.
Tetrahedral ionic
92
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Determine the molecular geometry and molecular polarity for hydrogen sulfide.
Bent nonpolar
93
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Determine the molecular geometry and molecular polarity for HCN.
Linear nonpolar
94
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Determine the molecular geometry and molecular polarity for SiH4.
Tetrahedral nonpolar
95
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Determine the molecular geometry and molecular polarity for nitrogen trichloride.
Trigonal pyramidal nonpolar
96
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How many total valence electrons does antimony (III) chloride have?
8
29
26
12
15
8
29
26
12
15
26
97
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What is the molecular geometry and molecular polarity for NBr3?
Trigonal pyramidal nonpolar
98
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Molecular polarity is determined by:
Molecular geometry, molecular symmetry and electronegativity difference
99
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What is the molecular geometry and molecular polarity for OF2?
Bent polar
100
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The geometry of a molecule is determined by:
The Lewis structure bonding electron pairs and lone pairs around the central atom.
