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A homogeneous mixture that does not settle out upon standing is
a colloid.
homogeneous.
an element.
hydrated.
a suspension.
a colloid.
A solution is prepared by dissolving 2 g of KCl in 100 g of H2O. In this solution, H2O is the
solid.
solution.
solvent.
solute.
ionic compound.
solvent
In a solution, the solvent
can be a solid, liquid, or gas.
is never a solid.
is the substance present in the smallest concentration.
can be a liquid or gas.
is a liquid.
can be a solid, liquid, or gas.
When KCl dissolves in water
the K+ ions are attracted to Cl- ions on the KCl crystal.
the Cl- ions are attracted to dissolved K+ ions.
the Cl- ions are attracted to the partially negative oxygen atoms of the water molecule.
the K+ ions are attracted to the partially positive hydrogen atoms of the water molecule.
the K+ ions are attracted to the partially negative oxygen atoms of the water molecule.
the K+ ions are attracted to the partially negative oxygen atoms of the water molecule.
Oil does not dissolve in water because
water is saturated.
oil is polar.
oil is nonpolar.
water is nonpolar.
oil is hydrated.
oil is nonpolar.
Water is a polar solvent and hexane (C6H14) is a nonpolar solvent. Which of the following correctly describes the solubility of the solute?
CaCl2, soluble in hexane
mineral oil, soluble in water
CCl4 , soluble in water
NaHCO3, soluble in water
octane, soluble in water
NaHCO3, soluble in water
A hydrogen bond is
a covalent bond between H and O.
an ionic bond between H and another atom.
a bond that is stronger than a covalent bond.
the polar O-H bond in water.
an attraction between a hydrogen atom attached to N, O, or F and an N, O, or F atom on another molecule.
an attraction between a hydrogen atom attached to N, O, or F and an N, O, or F atom on another molecule.
The O-H bond in water is polar because
it is an ionic bond.
it is a hydrogen bond.
oxygen occupies more space than hydrogen.
oxygen is much more electronegative than hydrogen.
hydrogen is much more electronegative than oxygen.
oxygen is much more electronegative than hydrogen.
Which of the following molecules can form hydrogen bonds?
NaH
HI
BH3
CH4
NH3
NH3
In water, a substance that ionizes completely in solution is called a
nonelectrolyte.
nonconductor.
weak electrolyte.
strong electrolyte.
semiconductor.
strong electrolyte
Choose the statement below that is TRUE.
A weak acid solution consists of mostly nonionized acid molecules.
A molecular compound that does not ionize in solution is considered a strong electrolyte.
The term "weak electrolyte" means that the substance is inert.
The term "strong electrolyte" means that the substance is extremely reactive.
A strong acid solution consists of only partially ionized acid molecules.
A weak acid solution consists of mostly nonionized acid molecules.
Which of the following solutions will have the highest electrical conductivity?
0.045 M Al 2(SO 4) 3
0.10 M LiBr
0.10 M NaI
0.050 M (NH 4) 2CO 3
0.10 M KF
0.045 M Al 2(SO 4) 3
In water, a substance that partially ionizes in solution is called a
semiconductor.
nonconductor.
nonelectrolyte.
weak electrolyte.
strong electrolyte.
weak electrolyte.
Which of the following is considered a STRONG electrolyte?
NH 4NO 3
HC 2H 3O 2
PbCl 2
C 12H 22O 11
CH 3OH
NH 4NO 3
Identify acetic acid.
weak electrolyte, strong acid
strong electrolyte, weak acid
nonelectrolyte
weak electrolyte, weak acid
strong electrolyte, strong acid
weak electrolyte, weak acid
Identify NaCl.
strong electrolyte
nonelectrolyte
weak electrolyte
weak acid
strong acid
strong electrolyte
Identify sugar.
strong electrolyte, weak acid
strong electrolyte, strong acid
nonelectrolyte
weak electrolyte, weak acid
weak electrolyte, strong acid
nonelectrolyte
Identify HCl.
weak electrolyte, weak acid
nonelectrolyte
weak electrolyte, strong acid
strong electrolyte, strong acid
strong electrolyte, weak acid
strong electrolyte, strong acid
Which of the following is NOT a strong electrolyte?
Li 2SO 4
MgCO 3
NaC 2H 3O 2
CaCl 2
LiOH
MgCO 3
1.0 mole of NaCl is added to 1.0 L of water. The freezing point of the solution will be __________ the freezing point of pure water.
higher than
the same as
lower than
lower than
An increase in the temperature of a solution usually
increases the solubility of a gas in the solution.
increases the boiling point.
decreases the solubility of a liquid solute in the solution.
decreases the solubility of a solid solute in the solution.
increases the solubility of a solid solute in the solution.
increases the solubility of a solid solute in the solution.
When some of the sugar added to iced tea remains undissolved at the bottom of the glass, the solution is
nonpolar.
unsaturated.
polar.
saturated.
dilute.
saturated.
The solubility of KI is 50 g in 100 g of H 2O at 20 °C. If 110 grams of KI are added to 200 grams of H 2O,
the solution will freeze.
all of the KI will dissolve.
the solution will start boiling.
a saturated solution will form.
the solution will be unsaturated.
a saturated solution will form.
According to Henry's law, the solubility of a gas in a liquid
depends on the liquid density.
decreases as the gas pressure above the liquid increases.
depends on the liquid polarity.
remains the same as the temperature increases.
increases as the gas pressure above the liquid increases.
increases as the gas pressure above the liquid increases.
Which one of the following compounds will NOT be soluble in water?
NaOH
K2SO4
PbS
MgCl2
LiNO3
PbS
How many of the following compounds are insoluble in water?
KC 2H 3O 2
CaSO 4
SrS
AlPO 4
4
0
1
2
3
2
How many of the following compounds are soluble in water?
Cu(OH) 2
LiNO 3
NH 4Br
K 2S
1
4
3
2
0
3
Which of the following compounds is soluble in water?
BaSO4
CaS
MgCO3
PbCl2
None of these compounds is soluble in water.
CaS
Which one of the following compounds will NOT be soluble in water?
LiOH
NaNO3
K2S
MgCl2
BaSO4
BaSO4
Which of the following compounds is insoluble in water?
MgSO4
BaS
Hg2I2
(NH4)2CO3
All of these compounds are soluble in water.
Hg2I2
Which one of the following compounds will be soluble in water?
LiCl
CaSO4
PbCO3
AgCl
Cu(OH)2
LiCl
Which one of the following compounds will be soluble in water?
PbS
AgBr
NH4Cl
CaCO3
Ca(OH)2
NH4Cl
Which of the following is a precipitation reaction?
Zn(s) + 2 AgNO 3(aq) → 2 Ag(s) + Zn(NO 3) 2(aq)
2 LiI(aq) + Hg 2(NO 3) 2(aq) → Hg 2I 2(s) + 2 LiNO 3(aq)
NaCl(aq) + LiI(aq) → NaI(aq) + LiCl(aq)
HCl(aq) + KOH(aq) → KCl(aq) + H 2O(l)
None of the above are precipitation reactions.
2 LiI(aq) + Hg 2(NO 3) 2(aq) → Hg 2I 2(s) + 2 LiNO 3(aq)
What precipitate is most likely formed from a solution containing Ba +2, Na +1, OH -1, and CO 3 -2.
NaOH
Ba(OH) 2
BaCO 3
Na 2CO 3
BaCO 3
When solutions of NaCl and AgNO 3 are mixed,
a precipitate of AgCl 2 forms.
a precipitate of NaNO 3 forms.
no precipitate forms.
precipitate of NaNO 3 and AgCl form.
a precipitate of AgCl forms.
a precipitate of AgCl forms.
Which of the following pairs of aqueous solutions will form a precipitate when mixed?
Li 2S + HCl
HCl + LiOH
K 2CO 3 + HNO 3
MgCl 2 + KOH
All of these solution pairs will produce a precipitate.
MgCl 2 + KOH
Which of the following pairs of aqueous solutions will form a precipitate when mixed?
(NH 4) 2SO 4 + LiCl
KNO 3 + NaOH
Sr(C 2H 3O 2) 2 + Na 2SO 4
LiOH + Na 2S
None of the above solution pairs will produce a precipitate.
Sr(C 2H 3O 2) 2 + Na 2SO 4
Which of the following pairs of aqueous solutions will form a precipitate when mixed?
CaS + Na2SO4
Na2 SO4 + KOH
K2CO3 + NaCl
None of these solution pairs will produce a precipitate.
All of these solution pairs will produce a precipitate.
CaS + Na2SO4
Identify the spectator ions in the following molecular equation.
KBr(aq) + AgNO 3(aq) → AgBr(s) + KNO 3(aq)
Ag + and NO 3 -
Ag + and Br -
K + and Br -
K + and NO 3 -
There are no spectator ions in this reaction.
K + and NO 3 -
Which of the following pairs of aqueous solutions will form a precipitate when mixed?
NaCl + Li3PO4
AgC2H3O2 + Cu(NO3)2
NH4NO3 + Li2CO3
Hg2(NO3)2 + LiI
None of the above solution pairs will produce a precipitate.
Hg2(NO3)2 + LiI
Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Al(C 2H 3O 2) 3 and LiNO 3 are mixed.
Li +(aq) + C 2H 3O 2 -(aq) → LiC 2H 3O 2(s)
Al 3+(aq) + 3 NO 3 -(aq) + Li +(aq) + C 2H 3O 2 -(aq) → Al(NO 3) 3(aq) + LiC 2H 3O 2(s)
3 Li +(aq) + (C 2H 3O 2) 3 3-(aq) → Li 3(C 2H 3O 2) 3 (s)
Al 3+(aq) + 3 NO 3 -(aq) → Al(NO 3) 3(s)
No reaction occurs.
No reaction occurs.
Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of lithium sulfide and copper (II) nitrate are mixed.
2 Li +(aq) + S 2-(aq) + Cu 2+(aq) + 2 NO 3 -(aq) → Cu 2+(aq) + S 2-(aq) + 2 LiNO 3(s)
2 Li +(aq) + S 2-(aq) + Cu 2+(aq) + 2 NO 3 -(aq) → CuS(s) + 2 Li +(aq) + 2 NO 3 -(aq)
Li + (aq) + S -(aq) + Cu +(aq) + NO 3 -(aq) → CuS(s) + LiNO 3(aq)
Li + (aq) + SO 4 2-(aq) + Cu +(aq) + NO 3 -(aq) → CuS(s) + Li +(aq) + NO 3 -(aq)
No reaction occurs.
2 Li +(aq) + S 2-(aq) + Cu 2+(aq) + 2 NO 3 -(aq) → CuS(s) + 2 Li +(aq) + 2 NO 3 -(aq)
Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of H 2SO 4 and KOH are mixed.
H +(aq) + OH -(aq) → H 2O(l)
2 K +(aq) + SO 4 2-(aq) → K 2SO 4(s)
H 2 2+(aq) + OH -(aq) → H 2(OH) 2(l)
H +(aq) + OH -(aq) + 2 K +(aq) + SO 4 2-(aq) → H 2O(l) + K 2SO 4(s)
No reaction occurs.
H +(aq) + OH -(aq) → H 2O(l)
Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of K2S and Fe(NO3)2 are mixed.
K+(aq) + NO3-(aq) → KNO3(s)
Fe2+(aq) + S2-(aq) → FeS(s)
Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → FeS(s) + 2 K+(aq) + 2 NO3-(aq)
Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → Fe2+(aq) + S2-(aq) + 2 KNO3(s)
No reaction occurs.
Fe2+(aq) + S2-(aq) → FeS(s)
When solutions of KCl and Pb(NO3) 2 are mixed, a precipitate forms. Which of the following is the balanced equation for the double replacement reaction that occurs?
KNO3(aq) + PbCl2(s) → KCl(aq) + Pb(NO3) 2(aq)
KCl(aq) + Pb(NO3) 2(aq) → KNO3(aq) + PbCl2(s)
K+(aq) + NO3-(aq) → KNO3(aq)
2KCl (aq) + Pb(NO3) 2(aq) → 2 KNO3(aq) + PbCl2 (s)
KCl(aq) + Pb(NO3) 2(aq) → KNO3(aq) + PbCl(s)
2KCl (aq) + Pb(NO3) 2(aq) → 2 KNO3(aq) + PbCl2 (s)
The mass percent concentration refers to
grams of solute in 100 g of solvent.
grams of solute in 1 kg of solution.
grams of solute in 1 kg of solvent.
grams of solvent in 100 g of solution.
grams of solute in 100 g of solution.
grams of solute in 100 g of solution.
The mass/volume percent concentration refers to
grams of solute in 100 mL of solution.
grams of solute in 1 L of solvent.
grams of solute in 1 L of solution.
grams of solute in 100 mL of solvent.
grams of solvent in 100 mL of solution.
grams of solute in 100 mL of solution.
The molarity (M) of a solution refers to
moles of solute/L of solution.
grams of solute/L of solution.
moles of solute/100 mL of solution.
grams of solute/100 mL of solution.
moles of solute/L of solvent.
moles of solute/L of solution.
Which of the following solutions will have the highest concentration of chloride ions?
0.05 M CaCl2
0.10 M MgCl2
0.10 M NaCl
0.10 M AlCl3
All of these solutions have the same concentration of chloride ions.
0.10 M AlCl3
During the process of diluting a solution to a lower concentration,
there is more solute in the concentrated solution.
the volume of the solution does not change.
water is removed from the concentrated solution.
the amount of solute does not change.
the amount of solvent does not change.
the amount of solute does not change.
In any chemical reaction, the rate of the reaction can be increased by
adding product molecules to the reaction mixture.
increasing the concentrations of the reactants.
changing the size of the container.
decreasing the temperature.
adding water to the reaction.
increasing the concentrations of the reactants.
In a catalyzed chemical reaction, one function of a catalyst is to
increase the number of successful reactant collisions.
change the equilibrium concentrations of the products and reactants.
increase the temperature at which the reaction is carried out.
decrease the concentration of reactants.
increase the energy given off during the reaction.
increase the number of successful reactant collisions.
The rate of any chemical reaction can be determined by observing
the theoretical yield of the reaction.
the amount of product formed in a unit of time.
the number of chemical bonds broken and remade.
the ratio of product concentration to reactant concentration.
the percent composition of the final product.
the amount of product formed in a unit of time.
Refrigerating perishable foods affects biochemical reactions by
increasing concentrations of antioxidants.
improving the appearance of the foods.
catalyzing the removal of harmful chemicals from the foods.
removing bacteria.
decreasing the rate of reactions affecting spoilage.
decreasing the rate of reactions affecting spoilage.
In an exothermic reaction, heat can be considered a __________.
catalyst
reactant
product
rate
determinant
product
A catalyst is
a substance that speeds up a reaction without being consumed in the reaction.
a product in a chemical reaction.
a reactant in a chemical reaction.
a substance that increases the energy of the products.
a substance that decreases the energy of the products.
a substance that speeds up a reaction without being consumed in the reaction.
The activation energy of a chemical reaction is the energy that
must be released from the mixture.
is the difference in the energies of the starting materials and products.
activates the catalyst.
initiates the reaction.
must be removed from the mixture.
initiates the reaction.
When a reaction is at equilibrium,
no more reactants are converted to products.
all reaction stops.
the reaction is no longer reversible.
the products and reactants have the same energy content.
the forward and reverse reactions occur at the same rate.
the forward and reverse reactions occur at the same rate.
A chemical reaction has reached equilibrium when
the rate of the forward reaction equals the rate of the reverse reaction.
all products have been removed from the reaction mixture.
all reactants have been converted to products.
the catalyst has been used up.
the concentrations of reactants and products are equal.
the rate of the forward reaction equals the rate of the reverse reaction.
A reaction that can proceed in either the forward or the reverse direction as written is called a __________ reaction.
reversible
favored
microscopic
solid phase
miniscule
reversible
An equilibrium in which all the components are gases is a __________ equilibrium.
heterogeneous
liquid
homogeneous
reversible
catalytic
homogeneous
For the reaction of carbon with carbon dioxide to make carbon monoxide, the reaction is as follows.
C(s) + CO2(g) 2CO(g)
This is an example of a __________ equilibrium.
homogeneous
gas
catalytic
irreversible
heterogeneous
heterogeneous
The reaction for the decomposition of PCl 5 to chlorine and PCl 3 is shown below.
PCl 5( g) PCl 3( g) + Cl 2( g)
If the equilibrium concentrations are [PCl 5] = 1.0 M, [PCl 3] = 0.10 M, [Cl 2] = 0.10 M, what is the value of the equilibrium constant?
1.0 × 10 2
2.0 × 10 -2
1.0 × 10 -2
10 × 10 -2
1.0 × 10 -4
1.0 × 10 -2
Which of the following statements is FALSE?
K >> 1 implies that the reaction is very fast at producing products.
When K >> 1, the forward reaction is favored and essentially goes to completion.
When K ≈ 1, neither the forward or reverse reaction is strongly favored, and about the same amount of reactants and products exist at equilibrium.
When K << 1, the reverse reaction is favored and the forward reaction does not proceed to a great extent.
None of the above.
K >> 1 implies that the reaction is very fast at producing products.
The equilibrium constant for the production of carbon dioxide from carbon monoxide and oxygen is K=2×10^11 This means that the reaction mixture at equilibrium is likely to consist of
twice as much starting material as product.
mostly starting materials.
mostly products.
an equal mixture of products and reactants.
twice as much product as starting material.
mostly products.
Which of the following equilibrium constants indicates the reaction that gives the smallest amount of product?
Kc = 5 × 101
Kc = 5 × 10-10
Kc = 5 × 1010
Kc = 5 × 10-1
Kc = 5 × 100
Kc = 5 × 10-10
The value of the equilibrium constant for the combination of nitrogen and oxygen to make NO is 2 × 10-9. What does this tell you about the concentrations of materials in the equilibrium mixture?
The concentration of reactants exceeds the concentration of products.
The concentrations of reactants and products are equal.
The products are solids.
The concentration of products exceeds the concentration of reactants.
The reactants are solids.
The concentration of reactants exceeds the concentration of products.
In the following gas phase reaction, Kc is much less than 1. At equilibrium, which of the following statements is true?
COCl2(g) CO(g) + Cl2(g)
A catalyst will increase the concentration of products formed.
The concentration of reactant is much greater than the concentration of products.
At equilibrium, the concentrations of reactants and products are equal.
The concentration of products is much greater than the concentration of reactants.
The concentrations of products and reactants are approximately equal.
The concentration of reactant is much greater than the concentration of products.
The equilibrium for the reaction for the decomposition of PCl 5 to chlorine and PCl 3 is 0.042.
PCl 5( g) PCl 3( g)+ Cl 2( g)
If the equilibrium concentrations are [PCl 3] = 0.010 M, [Cl 2] = 0.10 M, what is the value of [PCl 5]?
0.0020 M
0.010 M
0.042 M
0.024 M
0.0010 M
0.024 M
For the reaction of carbon with carbon dioxide to make carbon monoxide, one set of conditions produced a Kc = 1.2 × 10 -1. At equilibrium at a certain temperature, the concentration of product was 0.60 M. What was the concentration of carbon dioxide at that temperature?
C( s) + CO 2( g) 2CO( g)
5.0 M
0.60 M
3.33 M
3.0 M
0.36 M
3.0 M
For the following reaction, the equilibrium constant Kc is 2.0 at a certain temperature. If the concentration of both products is 0.10 M at equilibrium, what is the concentration of the starting material, NOBr?
2NOBr(g) 2NO(g) + Br2(g)
2.2 × 10-4 M
2.2 × 10-2 M
2.2 M
5 × 10-4 M
5 × 10-2 M
2.2 × 10-2 M
For the following reaction, the equilibrium constant Kc is 2.0 at a certain temperature. The reaction is endothermic. What do you expect to happen to the concentration of NO if the temperature is doubled?
2NOBr( g) 2NO( g) + Br 2( g)
A catalyst will be needed to make a change in concentration.
The concentration of NO will decrease.
The concentration of NO will increase.
There will be no change in [NO].
The change in concentration of [NO] will depend on the size of the vessel.
The concentration of NO will increase.
For the following equilibrium reaction, which cause and effect are correctly matched?
CO( g) + 2H 2( g) CH 3OH( g) + heat
add heat, shift right
add CO, shift left
remove heat, no change
remove H 2, shift left
remove CH 3OH, shift left
remove H 2, shift left
For the following reaction, the equilibrium constant Kc is 2.0 at a certain temperature. Bromine can be liquefied easily and removed from the reaction vessel as it is formed. If this is done, how will it affect the equilibrium reaction?
2NOBr( g) 2NO( g) + Br 2( g)
The equilibrium constant will change.
More products will be made as Br 2 is removed.
The pressure in the vessel will increase.
There will be a larger proportion NOBr in the vessel when equilibrium is reached.
Less NO will be made.
More products will be made as Br 2 is removed.
For the reaction of carbon with carbon dioxide to make carbon monoxide, the reaction is as follows.
C( s) + CO 2( g) 2CO( g)
Adding additional C( s) to the reaction container will cause __________ to occur.
the formation of more CO
the formation of more CO 2
a decrease in the amount of CO
B and C
no change in the amounts of CO and CO 2
no change in the amounts of CO and CO 2
In a catalytic converter in an automobile, the reaction of carbon monoxide with oxygen produces __________.
carbon and more oxygen
nitrogen oxide
methane
water
carbon dioxide
carbon dioxide
In the following gas phase reaction, what is the effect of adding more NO2 to the starting reaction mixture?
2NO2(g) → N2O4(g)
It would slow the reaction down.
It would increase the final quantity of products.
It would make the reaction more exothermic.
It would decrease the final quantity of products.
It would make the reaction more endothermic.
It would increase the final quantity of products.
In the following gas phase reaction, what is the effect on the direction of the reaction if more SO3 is added to the reaction mixture?
2SO2(g) + O2(g) 2SO3(g)
The equilibrium shifts to produce more products.
The equilibrium shifts to produce more reactants.
The position of the equilibrium remains unchanged.
The catalyst for the reaction is used up.
The rate of formation of products is increased.
The equilibrium shifts to produce more reactants.
In the reaction of carbon dioxide with water to give carbonic acid, the only gaseous component is the carbon dioxide. What will happen to the equilibrium concentration of carbonic acid if the pressure of carbon dioxide is increased in the container?
The carbonic acid concentration will stay the same.
The carbonic acid concentration will decrease.
The concentration of carbonic acid will increase.
There will be more water available for the reaction.
There will be twice as much carbonic acid as carbon dioxide.
The concentration of carbonic acid will increase.
In the reaction of nitrogen gas with oxygen gas to produce nitrogen oxide, what is the effect of adding more oxygen gas to the initial reaction mixture? The reaction is shown below.
N2(g) + O2(g) 2NO(g)
The equilibrium is not affected.
Extra catalyst is required to reach equilibrium.
The temperature of the reaction mixture is raised.
The equilibrium shifts to produce more N2.
The equilibrium shifts to produce more NO.
The equilibrium shifts to produce more NO.
Iron metal reacts with oxygen gas to produce iron(III) oxide. What will be the effect of increasing the pressure of oxygen gas in a closed reaction vessel?
Less reaction will take place.
The reaction mixture will catch fire.
More iron oxide will be produced.
The rate of production of iron oxide will slow down.
There is no effect; a catalyst is needed.
More iron oxide will be produced.
PCl5 (g) PCl3 (g)+ Cl2 (g)
For the reaction at equilibrium, if the volume of the container is increased, the amount of PCl5 present will
triple.
increase.
double.
stay the same.
decrease.
decrease.
When you open a bottle of a soft drink and leave it open, the drink eventually goes flat. This happens because the equilibrium between carbonic acid and carbon dioxide shifts to produce
more water.
more carbonic acid.
more hydrogen ions.
more carbon dioxide.
more oxygen.
more carbon dioxide.
Consider the following reaction and its equilibrium constant:
SO 2(g) + NO 2(g) ⇌ SO 3(g) + NO(g) K c = 0.33
A reaction mixture contains 0.39 M SO 2, 0.14 M NO 2 , 0.11 M SO 3 and 0.14 M NO. Which of the following statements is TRUE concerning this system?
The reaction will shift in the direction of products.
The equilibrium constant will decrease.
The reaction quotient will decrease.
The reaction will shift in the direction of reactants.
The system is at equilibrium.
The reaction will shift in the direction of products.
Consider the following reaction and its equilibrium constant:
4 CuO(s) + CH 4(g) ⇌ CO 2(g) + 4 Cu(s) + 2 H 2O(g) K c = 1.10
A reaction mixture contains 0.22 M CH 4, 0.67 M CO 2 and 1.3 M H 2O. Which of the following statements is TRUE concerning this system?
The reaction will shift in the direction of products.
The reaction quotient will increase.
The equilibrium constant will increase.
The reaction will shift in the direction of reactants.
The system is at equilibrium.
The reaction will shift in the direction of reactants.
Consider the following reaction at equilibrium. What effect will adding 1 mole of Ar to the reaction mixture have on the system?
2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)
No effect will be observed.
The equilibrium constant will increase.
The reaction will shift to the right in the direction of products.
The reaction will shift to the left in the direction of reactants.
The equilibrium constant will decrease.
No effect will be observed.
Consider the following reaction at equilibrium. What effect will adding CO2 have on the system?
CO2(g) + C(graphite) ⇌ 2 CO(g)
The equilibrium constant will decrease.
No effect will be observed since C is not included in the equilibrium expression.
The reaction will shift to the left in the direction of reactants.
The reaction will shift to the right in the direction of products.
The equilibrium constant will increase.
The reaction will shift to the right in the direction of products.
Consider the following reaction at equilibrium. What effect will adding more H2S have on the system?
2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)
No change will be observed.
The equilibrium constant will decrease.
The reaction will shift in the direction of products.
The reaction will shift to the left.
The equilibrium constant will increase.
The reaction will shift in the direction of products.
Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system?
CuS(s) + O2(g) ⇌ Cu(s) + SO2(g)
No effect will be observed.
The equilibrium constant will decrease.
The reaction will shift to the left in the direction of reactants.
The equilibrium constant will increase.
The reaction will shift to the right in the direction of products.
No effect will be observed.
Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system?
2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)
The reaction will shift to the left in the direction of reactants.
The reaction will shift to the right in the direction of products.
The equilibrium constant will increase.
No effect will be observed.
The equilibrium constant will decrease.
The reaction will shift to the right in the direction of products.
Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system?
Fe3O4(s) + CO(g) ⇌ 3 FeO(s) + CO2(g) ΔH°= +35.9 kJ
The reaction will shift to the right in the direction of products.
The equilibrium constant will decrease.
The equilibrium constant will increase.
The reaction will shift to the left in the direction of reactants.
No effect will be observed.
The reaction will shift to the right in the direction of products.
Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system?
C3H8(g) + 5 O2(g) ⇌ 3 CO2(g) + 4 H2O(l) ΔH° = -2220 kJ
The reaction will shift to the right in the direction of products.
The reaction will shift to the left in the direction of reactants.
No effect will be observed.
The equilibrium constant will decrease.
The equilibrium constant will increase.
The reaction will shift to the left in the direction of reactants.
Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system?
Xe(g) + 2 F2(g) → XeF4(g)
The equilibrium constant will decrease.
The reaction will shift to the left in the direction of reactants.
The reaction will shift to the right in the direction of products.
No effect will be observed.
The equilibrium constant will increase.
The reaction will shift to the right in the direction of products.
Consider the following reaction at equilibrium. What effect will reducing the pressure of the reaction mixture have on the system?
Xe(g) + 2 F2(g) → XeF4(g)
No effect will be observed.
The equilibrium constant will decrease.
The reaction will shift to the left in the direction of reactants.
The reaction will shift to the right in the direction of products.
The equilibrium constant will increase.
The reaction will shift to the left in the direction of reactants.
Consider the following reaction at equilibrium. What effect will removing H2O have on the system?
2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)
The reaction will shift to the left.
The equilibrium constant will decrease.
The equilibrium constant will increase.
No change will be observed.
The reaction will shift in the direction of products.
The reaction will shift in the direction of products.
Consider the following reaction at equilibrium. What effect will removing NO2 have on the system?
SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)
The reaction will shift in the direction of reactants.
The reaction will shift in the direction of products.
The equilibrium constant will decrease.
The reaction will shift to decrease the pressure.
No change will occur since SO3 is not included in the equilibrium expression.
The reaction will shift in the direction of reactants.
Consider the following reaction at equilibrium. What effect will adding more SO 3 have on the system?
SO 2(g) + NO 2(g) ⇌ SO 3(g) + NO(g)
The reaction will shift to decrease the pressure.
No change will occur since SO 3 is not included in the equilibrium expression.
The reaction will shift in the direction of products.
The reaction will shift in the direction of reactants.
The equilibrium constant will decrease.
The reaction will shift in the direction of reactants.
Consider the following reaction at equilibrium. What effect will adding some C have on the system?
CO 2(g) + C(graphite) ⇌ 2 CO(g)
The reaction will shift to the right in the direction of products.
No effect will be observed since C is not included in the equilibrium expression.
The equilibrium constant will increase.
The equilibrium constant will decrease.
The reaction will shift to the left in the direction of reactants.
No effect will be observed since C is not included in the equilibrium expression.
Consider the following reaction at equilibrium. What effect will decreasing the temperature have on the system?
CO 2(g) + 2 H 2O(l) ⇌ CH 4(g) + 2 O 2(g) ΔH° = +890 kJ
No effect will be observed.
The reaction will shift to the left in the direction of reactants.
The equilibrium constant will increase.
The reaction will shift to the right in the direction of products.
The equilibrium constant will decrease.
The reaction will shift to the left in the direction of reactants.
Consider the following reaction at equilibrium. What effect will increasing the volume of the reaction mixture have on the system?
2 H 2S(g) + 3 O 2(g) ⇌ 2 H 2O(g) + 2 SO 2(g)
The reaction will shift to the left in the direction of reactants.
The reaction will shift to the right in the direction of products.
The equilibrium constant will increase.
The equilibrium constant will decrease.
No effect will be observed.
The reaction will shift to the left in the direction of reactants.
Note 
Flashcard (21)