Exam 2 Review - Chapters 7, 9, and 10

Practice flashcards created from lecture notes for Exam 2 covering key concepts from Chapters 7, 9, and 10.

What should you do to prepare for Exam 2?

Use the textbook to solve end-of-chapter problems and complete homework assignments before the due date.

How long do you have to complete Exam 2?

90 minutes.

How many questions are on Exam 2?

34 multiple choice and true/false questions plus 3 bonus questions.

What items do you need to bring for the exam?

Calculator (no cell phones allowed).

What materials will be provided during the exam?

Constants, Table with Solubility rules, and the Periodic Table.

What is the balanced equation for the reaction of K3PO4 and Ca(NO3)2?

2K3PO4 + 3Ca(NO3)2 → Ca3(PO4)2 + 6KNO3.

What coefficients balance BaCl2 and AgNO3 in their reaction?

1, 2, 2, 1.

What is the correct formula for lead(II) iodide?

PbI2.

What coefficient completes the balancing of C5H8 + ? O2 → 5CO2 + 4H2O?

7.

What is the coefficient of H2 when balancing Al + H2SO4 → Al2(SO4)3 + ? H2?

3.

What substance is produced when silver nitrate reacts with potassium chloride?

Potassium nitrate.

What type of reaction occurs when passing an electric current through water?

Decomposition reaction.

What type of reaction is 2C2H6 + 7O2 → 4CO2 + 6H2O?

Combustion reaction.

What products result from the reaction of MgCl2 and Na2CO3?

NaCl and MgCO3.

Which reaction is a combination reaction?

N2 + O2 → 2NO.

What are the products of the complete combustion of a hydrocarbon?

CO2 and H2O.

What is the balanced equation for the reaction of NaOH with H2SO4?

2NaOH + H2SO4 → Na2SO4 + 2H2O.

Which reaction is an oxidation-reduction reaction?

Zn + SO4 → ZnSO4 + H2.

What is the percent by mass of carbon in butanethiol (C4H8S)?

54%.

How many atoms are in a 0.600-mole sample of gold?

3.61 x 10^23 atoms.

How many moles of CO2 are in 88.0 grams of CO2?

2.00 moles.

What is the mass of 1.5 x 10^21 silicon atoms?

0.070 g.

Which of the following elements contains the largest number of moles in 10.0 g? (Na, C, Pb, Cu, Ne)

C (Carbon).

Which balloon has more atoms, 25 g of He or 25 g of Ne?

The helium balloon has more atoms.

How many molecules are in 78.0 g of SO3?

5.87 x 10^23 molecules.

What is the mass percent of carbon in oxalic acid (H2C2O4)?

26.7%.

Which compound has the highest percent of oxygen?

MnO2.

How many grams of potassium are in a 42.7 g sample of potassium nitrate?

16.5 g.

How many grams of ore are needed to obtain 454.0 g of iron? (Ore is 35.00% Fe)

1297 g.

What is the empirical formula of a compound containing 83 g potassium and 17 g oxygen?

K2O.

What is the molecular formula of a compound with a molar mass of and empirical formula C2H7?

C14H42.

What is the conversion factor for moles of Fe to moles of Fe2O3?

4Fe → 2Fe2O3.

How many moles of hydrogen are needed with 1.22 mol of N2 to form ammonia?

3.66 moles.

How many moles of oxygen are needed to react with 4.00 mol of Mg?

2.00 mol.

How many grams of Li3N can be made with 1.75 moles of Li?

20.3 g.

How many moles of oxygen are needed to produce 2.33 moles of water?

4.14 moles.

How many molecules of H2S are required to form 79.0 g of sulfur?

9.89 x 10^23 molecules.

What is the percent yield if 16.0 g of aluminum oxide is produced from 10.0 g of Al and 19.0 g of O2?

84.7%.

What is the theoretical yield of HCl from 60.0 g of BCl3 and 37.5 g of H2O?

56.0 g.

What is the percent yield when 28.16 g of CO2 is formed?

25.00%.

What type of reaction absorbs 150 kcal of energy?

Endothermic reaction.

What is the amount of CO2 produced from 12.4 g of carbonic acid?

8.80 g.

How many moles of O2 are consumed when burning 1.90 mol of magnesium?

0.950 moles.

If the reaction shown is exothermic, what is the energy level of the reactants?

Higher than that of the products.

Which substance is not a solution?

Copper.

How is oxygen classified in the air?

As the solute in a homogeneous gas mixture.

Which compound is least soluble in water?

N2.

What must be true for a solute to dissolve?

The solute-solvent forces must be greater than the solute-solute forces.

Which is a strong electrolyte?

All of the above (HCl, NaCl, NCl).

What is the solubility of solids in water?

Increases with increasing temperature.

How can gas solubility in liquid be increased?

By increasing the pressure of the gas above the solvent.

What is the mass percent of sugar in a 200 g water solution with 2.45 g of sugar?

1.21%.

What is the mass percent of ammonium carbonate solution? (Prepare from ? g solid in ? g water)

45.7%.

What is the molarity of a solution made with ? g of NaI in ? L?

0.286 M.

How to prepare a 2.50 M NaCl solution with 0.325 moles of NaCl?

You must prepare 130.0 mL of solution.

How many moles of KOH are in 750 mL of 5.00 M KOH?

3.75 moles.

How many grams of KCl are needed for ? g of KCl?

91.3 g.

The concentration of BaCl2 in a 0.15 M solution contains:

0.15 M Ba2+ ions and 0.30 M Cl- ions.

What must be true after diluting a solution?

The new solution has more volume but a lower concentration.

What is the final concentration after diluting to a certain volume?

0.350 M.

How much of a 12.0 M HCl is required to make 75 mL of 3.50 M HCl?

21.9 mL.

Which statement about colligative properties is false?

All of the statements are true.

Why is it not good to drink seawater?

The high salt concentration forces water out of the body.

What is osmotic pressure?

The pressure required to prevent solvent flow from high to low solute concentration.

What is the relationship between H2SO3 and H2SO4?

They are not a conjugate acid-base pair.

Which ions constitute a conjugate acid-base pair?

NH4+ and NH3.

What defines a strong acid?

One that completely dissociates in solution.

Is a strong acid always concentrated?

No.

What pH does a solution with a pH of 8.5 have?

It is a weak base.

What is the Arrhenius definition of acid?

Produces H+ in solution.

What is the Bronsted-Lowry definition of a base?

A proton acceptor.

Which is the conjugate acid of OH?

H2O.

Which is not an acid-base conjugate pair?

H2S and OH-.

In the reaction involving NH4+ and H2O, what is NH4+ classified as?

An acid.

What is a substance acting as both an acid and a base called?

Amphoteric.

What are the products of a neutralization reaction between KOH and H2SO4?

H2O and K2SO4.

What is the concentration of NaOH if a titration with 0.105 M HCl is performed?

0.0833 M.

Which of the following acids is diprotic?

H2SO4.

What is the concentration of hydroxide ions when the hydronium ion concentration is known?

6.7 x 10^-4 M.

What is the concentration of hydronium ions given hydroxide is 2.31 × 10^-4 M?

4.33 x 10^-11 M.

How should an acidic solution's conditions be compared?

[H3O+] greater than [OH-].

What is the pH of a solution with a certain hydronium concentration?

4.77.

What is the [H+] in a solution with a pH of 3.35?

4.5 × 10^-4 M.

What is the pOH for a solution with a given OH- concentration?

9.89.

Which statements are true of buffer solutions?

1 and 3 only.

Which combination creates a buffer solution?

Acetic acid and sodium acetate.