Question 1

A __________ ΔH corresponds to an __________ process.

Accepted Answer

A) negative, endothermic 
B) positive, exothermic 
C) positive, endothermic 
D) zero, exothermic 
E) zero, endothermic 
A) negative, endothermic 
B) positive, exothermic 
C) positive, endothermic 
D) zero, exothermic 
E) zero, endothermic

Question 2

Calculate the kinetic energy in J of an electron moving at 6.00 × 106 m/s. The mass of an electron is 9.11 × 10-28 g.

Accepted Answer

A) 4.98 × 10-48 
B) 3.28 × 10-14 
C) 1.64 × 10-17 
D) 2.49 × 10-48 
E) 6.56 × 10-14 
A) 4.98 × 10-48 
B) 3.28 × 10-14 
C) 1.64 × 10-17 
D) 2.49 × 10-48 
E) 6.56 × 10-14

Question 3

The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J)is required to raise the temperature of 15 g of lead from 22 °C to 37 °C?

Accepted Answer

A) 2.0 
B) -0.13 
C) 5.8 × 10-4 
D) 29 
E) 0.13 
A) 2.0 
B) -0.13 
C) 5.8 × 10-4 
D) 29 
E) 0.13

Question 4

The value of ΔH° for the reaction below is -1107 kJ: 2Ba (s)+ O2 (g)→ 2BaO (s)
How many kJ of heat are released when 15.75 g of Ba (s)reacts completely with oxygen to form BaO (s)?

Accepted Answer

A) 20.8 
B) 63.5 
C) 114 
D) 70.3 
E) 35.1 
A) 20.8 
B) 63.5 
C) 114 
D) 70.3 
E) 35.1

Question 5

Calculate the kinetic energy in joules of a 150 lb jogger (68.1 kg)traveling at 12.0 mile/hr (5.36 m/s).

Accepted Answer

A) 1.96 × 103 
B) 365 
C) 978 
D) 183 
E) 68.1 
A) 1.96 × 103 
B) 365 
C) 978 
D) 183 
E) 68.1

Question 6

The value of ΔH° for the reaction below is -336 kJ. Calculate the heat (kJ)released to the surroundings when 23.0 g of HCl is formed. CH4 (g)+ 3 Cl2 (g)→ CHCl3 (l)+ 3HCl (g)

Accepted Answer

A) 177 
B) 2.57 × 103 
C) 70.7 
D) 211 
E) -336 
A) 177 
B) 2.57 × 103 
C) 70.7 
D) 211 
E) -336

Question 7

A sample of iron absorbs 67.5 J of heat, upon which the temperature of the sample increases from 21.5 °C to 28.5 °C. If the specific heat of iron is 0.450 J/g-K, what is the mass (in grams)of the sample?

Accepted Answer

A) 4.3 
B) 11 
C) 21 
D) 1100 
E) 1.1 x 103 
A) 4.3 
B) 11 
C) 21 
D) 1100 
E) 1.1 x 103

Question 8

The value of ΔH° for the reaction below is -482 kJ. Calculate the heat (kJ)released to the surroundings when 6.00 g of CO (g)reacts completely. 2CO (g)+ O2 (g)→ 2CO2 (g)

Accepted Answer

A) 1450 
B) 103 
C) 51.6 
D) 482 
E) -482 
A) 1450 
B) 103 
C) 51.6 
D) 482 
E) -482

Question 9

A slice of apple pie contains 14.0 grams of fat, 2.00 grams of protein, and 52.0 grams of carbohydrate. The respective fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. If cycling typically burns 1000.0 kJ/hour, __________ minutes of cycling are required to completely burn off the slice of pie.

Accepted Answer

A) 1.45 
B) 4.66 
C) 8.25 
D) 87.0 
E) less than one minute 
A) 1.45 
B) 4.66 
C) 8.25 
D) 87.0 
E) less than one minute

Question 10

The specific heat capacity of solid copper metal is 0.385 J/g-K. How many joules of heat are needed to raise the temperature of a 1.55-kg block of copper from 33.0 °C to 77.5 °C?

Accepted Answer

A) 1.79 × 105 
B) 26.6 
C) 2.66 × 104 
D) 5.58 × 10-6 
E) 0.00558 
A) 1.79 × 105 
B) 26.6 
C) 2.66 × 104 
D) 5.58 × 10-6 
E) 0.00558

Question 11

Given the following reactions Fe2O3 (s)+ 3CO (s)→ 2Fe (s)+ 3CO2 (g)ΔH = -28.0 kJ
3Fe (s)+ 4CO2 (s)→ 4CO (g)+ Fe3O4 (s)ΔH = +12.5 kJ
The enthalpy of the reaction of Fe2O3 with CO
3 Fe2O3 (s)+ CO (g)→ CO2 (g)+ 2 Fe3O4 (s)
Is __________ kJ.

Accepted Answer

A) -59.0 
B) 40.5 
C) -15.5 
D) -109 
E) +109 
A) -59.0 
B) 40.5 
C) -15.5 
D) -109 
E) +109

Question 12

Given the data in the table below, ΔH°rxn for the reaction PCl3 (g)+ 3 HCl (g)→ 3 Cl2 (g)+ PH3 (g)
Is __________ kJ.

Accepted Answer

A) -570.37 
B) -385.77 
C) 570.37 
D) 385.77 
E) The ΔH°f of Cl2 (g)is needed for the calculation. 
A) -570.37 
B) -385.77 
C) 570.37 
D) 385.77 
E) The ΔH°f of Cl2 (g)is needed for the calculation.

Question 13

Given the following reactions: 2S (s)+ 3O2 (g)→ 2SO3 (g)ΔH = -790 kJ
S (s)+ O2 (g)→ SO2 (g)ΔH = -297 kJ
The enthalpy of the reaction in which sulfur dioxide is oxidized to sulfur trioxide
2SO2 (g)+ O2 (g)→ 2SO3 (g)
Is __________ kJ.

Accepted Answer

A) 196 
B) -196 
C) 1087 
D) -1384 
E) -543 
A) 196 
B) -196 
C) 1087 
D) -1384 
E) -543

Question 14

Which of the following is a statement of Hess's law?

Accepted Answer

A) If a reaction is carried out in a series of steps, the ΔH for the reaction will equal the sum of the enthalpy changes for the individual steps. 
B) If a reaction is carried out in a series of steps, the ΔH for the reaction will equal the product of the enthalpy changes for the individual steps. 
C) The ΔH for a process in the forward direction is equal in magnitude and opposite in sign to the ΔH for the process in the reverse direction. 
D) The ΔH for a process in the forward direction is equal to the ΔH for the process in the reverse direction. 
E) The ΔH of a reaction depends on the physical states of the reactants and products. 
A) If a reaction is carried out in a series of steps, the ΔH for the reaction will equal the sum of the enthalpy changes for the individual steps. 
B) If a reaction is carried out in a series of steps, the ΔH for the reaction will equal the product of the enthalpy changes for the individual steps. 
C) The ΔH for a process in the forward direction is equal in magnitude and opposite in sign to the ΔH for the process in the reverse direction. 
D) The ΔH for a process in the forward direction is equal to the ΔH for the process in the reverse direction. 
E) The ΔH of a reaction depends on the physical states of the reactants and products.

Question 15

The value of ΔH° for the reaction below is -1107 kJ: 2Ba (s)+ O2 (g)→ 2BaO (s)
How many kJ of heat are released when 5.75 g of BaO (s)is produced?

Accepted Answer

A) 56.9 
B) 23.2 
C) 20.8 
D) 193 
E) 96.3 
A) 56.9 
B) 23.2 
C) 20.8 
D) 193 
E) 96.3

Question 16

Given the following reactions N2 (g)+ 2 O2 (g)→ 2NO2 (g)ΔH = 66.4 kJ
2NO (g)+ O2 (g)→ 2NO2 (g)ΔH = -114.2 kJ
The enthalpy of the reaction of the nitrogen to produce nitric oxide
N2 (g)+ O2 (g)→ 2NO (g)
Is __________ kJ.

Accepted Answer

A) 180.6 
B) -47.8 
C) 47.8 
D) 90.3 
E) -180.6 
A) 180.6 
B) -47.8 
C) 47.8 
D) 90.3 
E) -180.6

Question 17

The specific heat of liquid bromine is 0.226 J/g-K. How much heat (J)is required to raise the temperature of 10.0 mL of bromine from 25.00 °C to 27.30 °C? The density of liquid bromine: 3.12 g/mL.

Accepted Answer

A) 5.20 
B) 16.2 
C) 300 
D) 32.4 
E) 10.4 
A) 5.20 
B) 16.2 
C) 300 
D) 32.4 
E) 10.4

Question 18

Coal contains hydrocarbons of high molecular weight as well as compounds containing ________, oxygen, or nitrogen.

Accepted Answer

The answer of Coal contains hydrocarbons of high molecular weight...

Question 19

The specific heat capacity of methane gas is 2.20 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of methane from 36.0 °C to 75.0 °C?

Accepted Answer

A) 88.6 
B) 429 
C) 1221 
D) 0.0113 
E) 22.9 
A) 88.6 
B) 429 
C) 1221 
D) 0.0113 
E) 22.9

Question 20

At what velocity (m/s)must a 20.0 g object be moving in order to possess a kinetic energy of 1.00 J?

Accepted Answer

A) 1.00 
B) 100 × 102 
C) 10.0 
D) 1.00 × 103 
E) 50.0 
A) 1.00 
B) 100 × 102 
C) 10.0 
D) 1.00 × 103 
E) 50.0

Exam 5: Thermochemistry

A __________ ΔH corresponds to an __________ process.

Calculate the kinetic energy in J of an electron moving at 6.00 × 106 m/s. The mass of an electron is 9.11 × 10-28 g.

The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J)is required to raise the temperature of 15 g of lead from 22 °C to 37 °C?

The value of ΔH° for the reaction below is -1107 kJ: 2Ba (s)+ O2 (g)→ 2BaO (s) How many kJ of heat are released when 15.75 g of Ba (s)reacts completely with oxygen to form BaO (s)?

Calculate the kinetic energy in joules of a 150 lb jogger (68.1 kg)traveling at 12.0 mile/hr (5.36 m/s).

The value of ΔH° for the reaction below is -336 kJ. Calculate the heat (kJ)released to the surroundings when 23.0 g of HCl is formed. CH4 (g)+ 3 Cl2 (g)→ CHCl3 (l)+ 3HCl (g)

A sample of iron absorbs 67.5 J of heat, upon which the temperature of the sample increases from 21.5 °C to 28.5 °C. If the specific heat of iron is 0.450 J/g-K, what is the mass (in grams)of the sample?

The value of ΔH° for the reaction below is -482 kJ. Calculate the heat (kJ)released to the surroundings when 6.00 g of CO (g)reacts completely. 2CO (g)+ O2 (g)→ 2CO2 (g)

The specific heat capacity of solid copper metal is 0.385 J/g-K. How many joules of heat are needed to raise the temperature of a 1.55-kg block of copper from 33.0 °C to 77.5 °C?

Given the following reactions Fe2O3 (s)+ 3CO (s)→ 2Fe (s)+ 3CO2 (g)ΔH = -28.0 kJ 3Fe (s)+ 4CO2 (s)→ 4CO (g)+ Fe3O4 (s)ΔH = +12.5 kJ The enthalpy of the reaction of Fe2O3 with CO 3 Fe2O3 (s)+ CO (g)→ CO2 (g)+ 2 Fe3O4 (s) Is __________ kJ.

Given the data in the table below, ΔH°rxn for the reaction PCl3 (g)+ 3 HCl (g)→ 3 Cl2 (g)+ PH3 (g) Is __________ kJ.

Given the following reactions: 2S (s)+ 3O2 (g)→ 2SO3 (g)ΔH = -790 kJ S (s)+ O2 (g)→ SO2 (g)ΔH = -297 kJ The enthalpy of the reaction in which sulfur dioxide is oxidized to sulfur trioxide 2SO2 (g)+ O2 (g)→ 2SO3 (g) Is __________ kJ.

Which of the following is a statement of Hess's law?

The value of ΔH° for the reaction below is -1107 kJ: 2Ba (s)+ O2 (g)→ 2BaO (s) How many kJ of heat are released when 5.75 g of BaO (s)is produced?

Given the following reactions N2 (g)+ 2 O2 (g)→ 2NO2 (g)ΔH = 66.4 kJ 2NO (g)+ O2 (g)→ 2NO2 (g)ΔH = -114.2 kJ The enthalpy of the reaction of the nitrogen to produce nitric oxide N2 (g)+ O2 (g)→ 2NO (g) Is __________ kJ.

The specific heat of liquid bromine is 0.226 J/g-K. How much heat (J)is required to raise the temperature of 10.0 mL of bromine from 25.00 °C to 27.30 °C? The density of liquid bromine: 3.12 g/mL.

Coal contains hydrocarbons of high molecular weight as well as compounds containing ________, oxygen, or nitrogen.

The specific heat capacity of methane gas is 2.20 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of methane from 36.0 °C to 75.0 °C?

At what velocity (m/s)must a 20.0 g object be moving in order to possess a kinetic energy of 1.00 J?

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

A ΔH corresponds to an process.

Calculate the kinetic energy in J of an electron moving at 6.00 × 10⁶ m/s. The mass of an electron is 9.11 × 10^-28g.

The value of ΔH° for the reaction below is -1107 kJ: 2Ba (s)+ O₂ (g)→ 2BaO (s) How many kJ of heat are released when 15.75 g of Ba (s)reacts completely with oxygen to form BaO (s)?

The value of ΔH° for the reaction below is -336 kJ. Calculate the heat (kJ)released to the surroundings when 23.0 g of HCl is formed. CH₄ (g)+ 3 Cl₂ (g)→ CHCl₃ (l)+ 3HCl (g)

The value of ΔH° for the reaction below is -482 kJ. Calculate the heat (kJ)released to the surroundings when 6.00 g of CO (g)reacts completely. 2CO (g)+ O₂ (g)→ 2CO₂ (g)

Given the following reactions Fe₂O₃ (s)+ 3CO (s)→ 2Fe (s)+ 3CO₂ (g)ΔH = -28.0 kJ 3Fe (s)+ 4CO₂ (s)→ 4CO (g)+ Fe₃O₄ (s)ΔH = +12.5 kJ The enthalpy of the reaction of Fe₂O₃ with CO 3 Fe₂O₃ (s)+ CO (g)→ CO₂ (g)+ 2 Fe₃O₄ (s) Is __________ kJ.

Given the data in the table below, ΔH°_rxn for the reaction PCl₃ (g)+ 3 HCl (g)→ 3 Cl₂ (g)+ PH₃ (g) Is __________ kJ.

Given the following reactions: 2S (s)+ 3O₂ (g)→ 2SO₃ (g)ΔH = -790 kJ S (s)+ O₂ (g)→ SO₂ (g)ΔH = -297 kJ The enthalpy of the reaction in which sulfur dioxide is oxidized to sulfur trioxide 2SO₂ (g)+ O₂ (g)→ 2SO₃ (g) Is __________ kJ.

The value of ΔH° for the reaction below is -1107 kJ: 2Ba (s)+ O₂ (g)→ 2BaO (s) How many kJ of heat are released when 5.75 g of BaO (s)is produced?

Given the following reactions N₂ (g)+ 2 O₂ (g)→ 2NO₂ (g)ΔH = 66.4 kJ 2NO (g)+ O₂ (g)→ 2NO₂ (g)ΔH = -114.2 kJ The enthalpy of the reaction of the nitrogen to produce nitric oxide N₂ (g)+ O₂ (g)→ 2NO (g) Is __________ kJ.