Problem Set II

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Question #1

In the reaction below, 8.0 g of H2 react with 7.0 g of O2. Which of the following statements is incorrect?
2 H2 + O2 → 2 H2O

A More moles of hydrogen are consumed than moles of oxygen.

B More moles of water are produced than moles of oxygen are consumed.

C More grams of oxygen are consumed than grams of hydrogen.

D More grams of hydrogen are consumed than grams of oxygen.

E More grams of water are produced than grams of oxygen are consumed.

Question #2

Determine the heat of reaction for the process
2 Fe(s) + 3/2 O2(g) → Fe2O3(s)
using the information given below:
2 Fe(s) + 6 H2O(l) → 2 Fe(OH)3(s) + 3 H2(g) Δ H° = +321.8 kJ

H2(g) + 1/2 O2(g) → H2O(l) Δ H° = −285.8 kJ

Fe2O3(s) + 3 H2O(l) → 2 Fe(OH)3(s) ΔH° = +288.6 kJ

A -824.2 kJ

B +252.6 kJ

C +324.6 kJ

D -247.0 kJ

E -252.6 kJ

Question #3

A solution is made by dissolving 60.0 g of AlCl3 in enough water to make 250.0 mL of solution. How many moles of chloride ions are in 5.00 mL of solution?

A 3.00 × 10−3 mol

B 1.80 × 10−2 mol

C 9.00 × 10−3 mol

D 1.25 × 10−3 mol

E 2.70 × 10−2 mol

Question #4

Arrange the following gaseous substances in order of decreasing average molecular speed at 25°C. argon, fluorine, carbon dioxide, oxygen, helium

A carbon dioxide > argon > fluorine > oxygen > helium

B carbon dioxide > fluorine > argon > oxygen > helium

C helium > oxygen > fluorine > carbon dioxide > argon

D argon > oxygen > helium > carbon dioxide > fluorine

E helium > oxygen > fluorine > argon > carbon dioxide

Question #5

What is the volume in mililiters of 2.361 g of nitrogen dioxide that occupies at 25.1°C and 3.1 atm of pressure?
R = 0.0821 L atm mol−1 K−1.

A 0.0405

B 4.0

C 0.075

D 0.41

E 4.1 x 102

Question #6

How many moles of ions are in 285 mL of 0.0150 M MgCl2?

A 1.28 × 10−2 mol

B 1.05 × 10−1 mol

C 5.26 × 10−1 mol

D 4.128 × 10−3 mol

E 5.26 × 10−2 mol

Question #7

If a 45.0 mL sample of 2.20 M Na2SO4 is diluted to yield a final solution that is 0.110 M in sodium ions, what is the volume of the final solution?

A 110 mL

B 450 mL

C 1800 mL

D 900 mL

E 4500 mL

Question #8

Calculate the number of moles of a gas that occupy 225 mL at STP. The value of R = 0.0821 L atm mol−1 K−1.

A 0.109

B Not solvable without the molar mass of the gas.

C 5.05 × 104

D 10.0

E 0.0100

Question #9

Determine the heat of reaction for the process
C2H4(g) + 6HCl(g) → 2CHCl3(g) + 4H2(g)
using the information given below:
2C(s) + 2H2(g) → C2H4(g) ΔH° = 52.3 kJ

H2(g) + Cl2(g) → 2HCl(g) Δ H° = −184.6kJ

C(s) + 1/2H2(g) + 3/2Cl2(g) → CHCl3(g) ΔH° = −103.1 kJ

A +29.2 kJ

B -29.2 kJ

C + 398.4 kJ

D + 295.3 kJ

E -295.3 kJ

Question #10

Write a balanced chemical equation for the exchange reaction that occurs when KOH(aq) is added to FeCl3(aq).

A KOH(aq) + FeCl3(aq) → FeOH(aq) + KCl(s)

B No reaction occurs.

C 3 KOH(aq) + FeCl3(aq) → K3Fe(s) + 3 HClO(aq)

D 3 KOH(aq) + FeCl3(aq) → Fe(OH)3(s) + 3 KCl(aq)

E KOH(aq) + FeCl3(aq) → FeOH(s) + KCl(aq)

Question #11

The Roman numerals in the reaction given represent the coefficients in the balanced chemical equation. What are the values of the coefficients?
I Fe3O4 + II H2 → III Fe + IV H2O

A 1 2 3 2

B 2 8 6 8

C 1 4 3 4

D 2 4 6 4

E 1 1 3 2

Question #12

A reaction has a theoretical yield of 38.73 g. It produces 18.81 g of product. Calculate the percent yield.

A 47.85%

B 47.78%

C 48.57%

D 46.50%

E 48.17%

Question #13

A cup of rice contain 110 Calories (dietary calories)? What is this energy in kJ (1 cal = 4.184 J)

A 26 kJ

B 4.6 × 105kJ

C 0.46 kJ

D 460 kJ

E 2.6 × 104 kJ

Question #14

Ammonia and sulfuric acid react according to the equation given below. How many milliliters of 0.110 M sulfuric acid are required to exactly neutralize 25.0 mL of 0.0840 M NH3 solution?
2 NH3(aq) + H2SO4(aq) → (NH4)2SO4(aq)

A 1.46 mL

B 3.64 mL

C 5.85 mL

D 1.82 mL

E 9.55 mL

Question #15

For the reaction given below, how many moles of aluminum will react if 12 moles of Br2 react and 8 moles of AlBr3 are produced?
2 Al + 3 Br2 → 2 AlBr3

A 40

B 4

C 16

D 12

E 8

Question #16

Which of the methods described below will yield 500 mL of a 0.100 M KMnO4 solution?

A Dissolve 15.8 g KMnO4 in water and dilute to exactly 500 mL.

B Add exactly 500 mL of water to 7.90 g of KMnO4.

C Dilute 220 mL of 1.00 M KMnO4 to exactly 500 mL.

D Add exactly 500 mL of water to KMnO4.

E Dissolve 7.90 g of KMnO4 in water and dilute to exactly 500 mL.

Question #17

What ions are present in an aqueous solution of lithium perchlorate, LiClO4(aq)?

A Li- and Cl+

B Li+ and ClO4-

C Li+, Cl-, and O2-

D Li+, Cl+, and O42-

E Li+ and Cl-

Question #18

A student mixes 10 g of an aqueous HCl solution with 10 g of an aqueous NaOH solution in a coffee-cup calorimeter and determines that the temperature change of the mixture upon heating was 3.0 C.

If the student calculated the heat using the equation: q = (20g)(4.184 J g-1 K-1)(3.0 K)

What assumptions are required for the value of the heat to be accurate?
I. the solution has the same specific heat as water
II the calorimeter absorbed little or no heat
III the initial temperature was 25 C

A II only

B All three assumptions are required

C I only

D II and III

E I and II

Question #19

How are the pressure and the absolute temperature of a gas related for a given number of moles at constant volume?

A They are indirectly proportional.

B Not enough information given to determine.

C They are exactly opposites.

D They are directly proportional.

E They are not related.

Question #20

How many grams of CO2 are produced from the reaction of 5.00 g of C2H6 with 25.0 g of O2?
2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

A 7.51 g

B 19.6 g

C 30.0 g

D 3.66 g

E 14.6 g

Question #21

In an endothermic reaction, heat is transferred from the _____________ to the _____________.

A surroundings, system

B atmosphere, ground

C system, surroundings

Question #22

A 25.00 mL sample of H3PO4 solution is neutralized by exactly 54.93 mL of 0.04345 M Ca(OH)2. What is the molarity of the H3PO4 solution?

A 0.09546 M

B 0.2148 M

C 0.0636 M

D 0.2897 M

E 0.1432 M

Question #23

A 64.05 mL sample of 0.250 M CH3COOH is to be exactly neutralized with 0.500 M KOH. How many milliliters of KOH will be required?

A 32.0 mL

B 64.1 mL

C 16.0 mL

D 128 ml

E 8.01 mL

Question #24

A hydrochloric acid (HCl) solution (25.00 m)L sample is neutralized by adding 31.22 mL of 0.08152 M Ca(OH)2. What is the molarity of the HCl solution?

A 0. 09453 M

B 0.1021 M

C 0.08152 M

D 0.2036 M

E 0.1018 M

Question #25

Which of the following represents oxidation?

A 2H+ + 2e− → H2

B F2 + 2e− → 2 F−

C Na → Na+ + e−

D Ni2+ + 2e− → Ni

E Mg2+ + 2e− → Mg

Question #26

In the reaction given below, how many grams of water are consumed if 4.0 g of hydrogen gas and 32.0 g of oxygen gas are produced? 2 H2O → 2 H2 + O2

A 2.0 g

B 20.0 g

C 36.0 g

D 18.0 g

E 4.0 g

Question #27

A mixture of H2(g) and Cl2(g) exerts a total pressure of 2.50 atm. If the mole fraction of H2 is 0.490, what is the partial pressure (in atm) of H2?

A 0.396

B 0.253

C 1.23

D 2.5

E 0.606

Question #28

What is the oxidation number of O in Fe2O3?

A −2

B −3

C +2

D +5

E −5

Question #29

How many kilojoules are there in 150 Calories of popcorn?

A 6.3 × 105 J

B 3.6 × 104 J

C 630 J

D 3.6 × 10−2 J

E 36 J

Question #30

The standard enthalpies of formation for several substances are given below:
CO(g) −110.5 kJ/mol CO2(g) −393.5 kJ/mol
H2O(l) −285.8 kJ/mol H2O(g) −241.8 kJ/mol
H2O2(l) −187.8 kJ/mol CH3OH(g) −200.7 kJ/mol
C2H5OH(l) −277.7 kJ/mol C2H5OH(g) −235.1 kJ/mol

Determine the ΔH° for the reaction below.
2CO(g) + 4H2(g) → C2H5OH(g) + H2O(g)

A −366.4 kJ

B −298.5 kJ

C −255.9 kJ

D −299.9 kJ

E 255.9 kJ

Question #31

A sample of 1.50 moles of ethanol (C2H5OH) is initially at 25.0°C. If the sample absorbs 3.00 kJ of heat, what is the final temperature of the ethanol? (specific heat of ethanol = 2.46 J g−1 °C−1)

A 62.5°C

B 42.6°C

C 7.35°C

D 30.2°C

E 838°C

Question #32

Convert 699 torr to 1) atm, 2) mmHg and 3) kPa.

A 699 5.31 × 105 5.24 × 103

B 0.920 699 9.32 × 104

C 5.31 × 105 5.31 × 105 93.2

D 0.920 699 93.2

E 6.90 6.995 × 105 7.08 × 104

Question #33

Which concept is not associated with the kinetic-molecular theory of gases?

A The sizes of gas molecules are small compared to the distances between the molecules.

B The average kinetic energy of gas molecules increases as the temperature increases.

C No energy is lost when gas molecules collide with each other.

D The velocity of a gas molecule is inversely proportional to its temperature.

E The forces of attraction and repulsion between separate gas molecules are minimal.

Question #34

The complete reaction of 16.12 g of titanium with 23.88 g of chlorine (Cl2) produces a compound with the formula TixCly. What is the empirical formula of the compound?

A TiCl

B Ti4Cl

C TiCl4

D TiCl2

E Ti2Cl

Question #35

A 125.0-mL contains a gas at 27°C and 760 mm Hg of pressure. The gas is pumped into an empty 1.50-L flask also at a temperature of 27°C. What is the pressure (in atm) of the gas in the new flask?

A 8.33 × 101

B 6.33 × 104

C none of these choices

D 6.33 × 101

E 8.33 × 10−2

Question #36

What is the maximum possible quantity of product obtained from a chemical reaction called?

A theoretical yield

B limiting reactant

C stoichiometric coefficients

D molecular weight of the product

E percent yield

Question #37

Based on the following thermochemical equation, which statement is false?
NH3(l) NH3(g) Δ H° = +23.4 kJ

A The pressure for the process is known.

B The thermochemical equation represents a physical change.

C The enthalpy change for the gas condensing into a liquid is known.

D The enthalpy change is endothermic.

E The internal energy of the surroundings increases.

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