Question 1

During a(n) ________ process, energy is transferred to the system from the surroundings.

Accepted Answer

A) exothermic 
B) endothermic 
C) thermodynamic 
D) thermochemical 
E) physical 
A) exothermic 
B) endothermic 
C) thermodynamic 
D) thermochemical 
E) physical

Question 2

Write the equation that corresponds to the standard enthalpy of formation for each of the following compounds: a) NaI(s), b) HClO4(g), and c) CH3OCH3(g)

Accepted Answer

a) Na(s) @#IMG-DLM& F1F1F1S1F1F1F10 @#IMG-DLM& I₂(s) F1F1F1S1

Question 3

A heating curve for some substance is shown below. Which of the line segments (I-V) represents heating of the liquid?

Accepted Answer

A) I 
B) II 
C) III 
D) IV 
E) V 
A) I 
B) II 
C) III 
D) IV 
E) V

Question 4

Determine the enthalpy for the following reaction, given F1F1F1S1F1F1F10F1F1F1S1F1F1F10   (NH3(g)) F1F1F1S1F1F1F10 F1F1F1S1F1F1F1046.1 kJ/mol,F1F1F1S1F1F1F10F1F1F1S1F1F1F10   (NO(g)) F1F1F1S1F1F1F10   F1F1F1S1F1F1F1090.3 kJ/mol, and F1F1F1S1F1F1F10F1F1F1S1F1F1F10   (H2O(g)) F1F1F1S1F1F1F10 F1F1F1S1F1F1F10241.8 kJ/mol. 4NH3(g)   F1F1F1S1F1F1F105O2(g)   F1F1F1S1F1F1F104NO(g)   F1F1F1S1F1F1F106H2O(g) F1F1F1S1F1F1F10Hrxn F1F1F1S1F1F1F10 ? kJ

Accepted Answer

A) (F1F1F1S1F1F1F101274 kJ/mol) 
B) (F1F1F1S1F1F1F101,996 kJ/mol) 
C) (F1F1F1S1F1F1F101,274 kJ/mol) 
D) (F1F1F1S1F1F1F10905.2 kJ/mol) 
E) (F1F1F1S1F1F1F10105.4 kJ/mol) 
A) (F1F1F1S1F1F1F101274 kJ/mol) 
B) (F1F1F1S1F1F1F101,996 kJ/mol) 
C) (F1F1F1S1F1F1F101,274 kJ/mol) 
D) (F1F1F1S1F1F1F10905.2 kJ/mol) 
E) (F1F1F1S1F1F1F10105.4 kJ/mol)

Question 5

Ethanol (CH3CH2OH) has been suggested as an alternative fuel source. Ethanol's enthalpy of combustion is F1F1F1S1F1F1F10Hcomb F1F1F1S1F1F1F10 F1F1F1S1F1F1F101,368 kJ/mol. What volume of ethanol (d F1F1F1S1F1F1F10 0.789 g/mL) is required to produce the same amount of energy as 1 gallon of gasoline, which can be modeled as isooctane (C8H18) with an energy density of 32.9 kJ/mL? (1 gal F1F1F1S1F1F1F10 3.785 L; d F1F1F1S1F1F1F10 0.703 g/mL)

Accepted Answer

A) 1.41 gal 
B) 1.00 gal 
C) 0.90 gal 
D) 0.85 gal 
E) 1.15 gal 
A) 1.41 gal 
B) 1.00 gal 
C) 0.90 gal 
D) 0.85 gal 
E) 1.15 gal

Question 6

According to the first law of thermodynamics, which of the changes A-D will always increase the internal energy of a system? (q = energy transferred, and w = work done)

Accepted Answer

A) q > 0, w  0, w > 0 
C) q  0 
E) None of the changes A-D will always increase the internal energy of a system. 
A) q > 0, w  0, w > 0 
C) q  0 
E) None of the changes A-D will always increase the internal energy of a system.

Question 7

In a steam engine, steam in a cylinder expands against a piston, exerting 10 atm of external pressure. The volume of the cylinder increases by 10 L and simultaneously the steam cools, losing 3,000 kJ of energy to the surroundings. What is the change in energy of the steam? (101.3 J F1F1F1S1F1F1F10 1 L atm)

Accepted Answer

A) (F1F1F1S1F1F1F103,010 kJ) 
B) (F1F1F1S1F1F1F103,001 kJ) 
C) (F1F1F1S1F1F1F103,100 kJ) 
D) (F1F1F1S1F1F1F1013,135 kJ) 
E) (F1F1F1S1F1F1F102,990 kJ) 
A) (F1F1F1S1F1F1F103,010 kJ) 
B) (F1F1F1S1F1F1F103,001 kJ) 
C) (F1F1F1S1F1F1F103,100 kJ) 
D) (F1F1F1S1F1F1F1013,135 kJ) 
E) (F1F1F1S1F1F1F102,990 kJ)

Question 8

The enthalpy of combustion of table sugar (sucrose, C12H22O11, 342.3 g/mol) is F1F1F1S1F1F1F105,643 kJ/mol. What is the food value (Cal/g) of sucrose? (1 Cal F1F1F1S1F1F1F10 4.184 kJ)

Accepted Answer

A) 3.94 Cal/g 
B) 11.1 Cal/g 
C) 16.5 Cal/g 
D) 2.92 Cal/g 
E) 1,350 Cal/g 
A) 3.94 Cal/g 
B) 11.1 Cal/g 
C) 16.5 Cal/g 
D) 2.92 Cal/g 
E) 1,350 Cal/g

Question 9

Benzoic acid is used to determine the heat capacity of bomb calorimeters because it can be obtained in pure form and its energy of combustion is known very accurately (F1F1F1S1F1F1F1026.43 kJ/g). Determine the heat capacity of a calorimeter that had a temperature increase of 9.199F1F1F1S1F1F1F10C when 3.500 g of benzoic acid was used.

Accepted Answer

A) 5.061 kJ/F1F1F1S1F1F1F10C 
B) 10.06 kJ/F1F1F1S1F1F1F10C 
C) 2.032 kJ/F1F1F1S1F1F1F10C 
D) 20.12 kJ/F1F1F1S1F1F1F10C 
E) 15.37 kJ/F1F1F1S1F1F1F10C 
A) 5.061 kJ/F1F1F1S1F1F1F10C 
B) 10.06 kJ/F1F1F1S1F1F1F10C 
C) 2.032 kJ/F1F1F1S1F1F1F10C 
D) 20.12 kJ/F1F1F1S1F1F1F10C 
E) 15.37 kJ/F1F1F1S1F1F1F10C

Question 10

A diver jumps off a diving board. At which point in the diagram below will the diver possess the greatest potential energy?

Accepted Answer

A) A 
B) B 
C) C 
D) D 
E) E 
A) A 
B) B 
C) C 
D) D 
E) E

Question 11

Assuming that the distances between the two ions are the same in all cases, which of the following ion pairs has the greatest electrostatic potential energy (i.e., largest in magnitude)?

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 12

According to Coulomb's law, which ionic compound A-D has the largest electrostatic potential energy (i.e., largest in magnitude)?

Accepted Answer

A) NaCl 
B) CaCl2 
C) AlCl3 
D) CoCl2 
E) All have the same potential energy because the chloride anions all have -1 charges. 
A) NaCl 
B) CaCl2 
C) AlCl3 
D) CoCl2 
E) All have the same potential energy because the chloride anions all have -1 charges.

Question 13

In an experiment, 30.0 g of metal was heated to 98.0F1F1F1S1F1F1F10C and then quickly transferred to 50.0 g of water in a calorimeter. The heat capacity of the calorimeter with the water was 211 J/F1F1F1S1F1F1F10C. The initial temperature of the calorimeter was 27.0F1F1F1S1F1F1F10C, and the final temperature after addition of the metal was 32.5F1F1F1S1F1F1F10C. What is the value of the specific heat capacity of the metal?

Accepted Answer

A) 0.140 J/(g F1F1F1S1F1F1F10 F1F1F1S1F1F1F10
C)  
B) 83.0 J/(g F1F1F1S1F1F1F10 F1F1F1S1F1F1F10
C)  
C) 0.540 J/(g F1F1F1S1F1F1F10 F1F1F1S1F1F1F10
C)  
D) 0.591 J/(g F1F1F1S1F1F1F10 F1F1F1S1F1F1F10
C)  
E) 29.5 J/(g F1F1F1S1F1F1F10 F1F1F1S1F1F1F10
C)  
A) 0.140 J/(g F1F1F1S1F1F1F10 F1F1F1S1F1F1F10
C)  
B) 83.0 J/(g F1F1F1S1F1F1F10 F1F1F1S1F1F1F10
C)  
C) 0.540 J/(g F1F1F1S1F1F1F10 F1F1F1S1F1F1F10
C)  
D) 0.591 J/(g F1F1F1S1F1F1F10 F1F1F1S1F1F1F10
C)  
E) 29.5 J/(g F1F1F1S1F1F1F10 F1F1F1S1F1F1F10
C)

Question 14

Suppose you eat a one-third pound hamburger without bread, cheese, or other items. Approximately how long would you need to walk to use up the calories in the hamburger? Assume the mass of the hamburger is 150 g with 3.6 Cal/g and that walking requires 2.5 times a basal metabolic rate of 280 kJ/hr.

Accepted Answer

A) 2 hours 
B) 3 hours 
C) 4 hours 
D) 5 hours 
E) 6 hours 
A) 2 hours 
B) 3 hours 
C) 4 hours 
D) 5 hours 
E) 6 hours

Question 15

Fuel density is ________

Accepted Answer

A) the cost of energy in kJ/$. 
B) the amount of energy contained in 1 mol of a substance (kJ/mol). 
C) the energy released when 1 g of a substance is burned (kJ/g). 
D) the energy released when 1 g of a substance is formed (kJ/g). 
E) the energy released when 1 L of a substance is burned (kJ/L). 
A) the cost of energy in kJ/$. 
B) the amount of energy contained in 1 mol of a substance (kJ/mol). 
C) the energy released when 1 g of a substance is burned (kJ/g). 
D) the energy released when 1 g of a substance is formed (kJ/g). 
E) the energy released when 1 L of a substance is burned (kJ/L).

Question 16

Which statement regarding combustion of a sample of gasoline in a bomb calorimeter is correct?

Accepted Answer

A) Work is done by the system on the surroundings. 
B) Work is done by the surroundings on the system. 
C) No work is done because the pressure is constant. 
D) The work done by the system equals the energy produced by the system. 
E) The experiment provides an accurate value for the change in energy, not the change in enthalpy. 
A) Work is done by the system on the surroundings. 
B) Work is done by the surroundings on the system. 
C) No work is done because the pressure is constant. 
D) The work done by the system equals the energy produced by the system. 
E) The experiment provides an accurate value for the change in energy, not the change in enthalpy.

Question 17

Ammonium nitrate sometimes is used in cold packs because its enthalpy of solvation in water is F1F1F1S1F1F1F1021 kJ/mol. What is the minimum amount of ammonium nitrate (80.05 g/mol) that is needed to cool a 1.0 L soft drink (d F1F1F1S1F1F1F10 1.0 g/mL, specific heat 4.5 J gF1F1F1S1F1F1F101   F1F1F1S1F1F1F10) and its plastic bottle (heat capacity 50 J/K) from 30   to 5   .

Accepted Answer

A) 540 g 
B) 320 g 
C) 110 g 
D) 430 g 
E) 250 g 
A) 540 g 
B) 320 g 
C) 110 g 
D) 430 g 
E) 250 g

Question 18

Given the following thermochemical equation detailing the combustion of glucose C6H12O6(s)   F1F1F1S1F1F1F106O2(g)   F1F1F1S1F1F1F10CO2(g)   F1F1F1S1F1F1F106H2O(g) F1F1F1S1F1F1F10Hrxn F1F1F1S1F1F1F10 F1F1F1S1F1F1F102803 kJ/mol C6F1F1F1S1F1F1F10H12O6
Determine the amount of glucose needed to release 30 kJ of energy.

Accepted Answer

A) 11.58 g 
B) 1.93 g 
C) 467 g 
D) 1,930 g 
E) 5.35 g 
A) 11.58 g 
B) 1.93 g 
C) 467 g 
D) 1,930 g 
E) 5.35 g

Question 19

How much work does a gas do when it expands against a constant pressure of 0.500 atm from a volume of 50.00 mL to a volume of 350.00 mL? (101.3 J F1F1F1S1F1F1F10 1 L atm)

Accepted Answer

A) 15.2 J 
B) 0.150 J 
C) (F1F1F1S1F1F1F1015.2 J) 
D) (F1F1F1S1F1F1F100.152 J) 
A) 15.2 J 
B) 0.150 J 
C) (F1F1F1S1F1F1F1015.2 J) 
D) (F1F1F1S1F1F1F100.152 J)

Question 20

The kinetic energy associated with the random motion of molecules is called ________

Accepted Answer

A) motional energy. 
B) work. 
C) heat. 
D) microscopic energy. 
E) thermal energy. 
A) motional energy. 
B) work. 
C) heat. 
D) microscopic energy. 
E) thermal energy.

During a(n) ________ process, energy is transferred to the system from the surroundings.

Write the equation that corresponds to the standard enthalpy of formation for each of the following compounds: a) NaI(s), b) HClO₄(g), and c) CH₃OCH₃(g)

A heating curve for some substance is shown below. Which of the line segments (I-V) represents heating of the liquid?

Determine the enthalpy for the following reaction, given  (NH₃(g))  46.1 kJ/mol, (NO(g))  90.3 kJ/mol, and  (H₂O(g))  241.8 kJ/mol. 4NH₃(g) 5O₂(g) 4NO(g) 6H₂O(g) H_rxn  ? kJ

According to the first law of thermodynamics, which of the changes A-D will always increase the internal energy of a system? (q = energy transferred, and w = work done)

In a steam engine, steam in a cylinder expands against a piston, exerting 10 atm of external pressure. The volume of the cylinder increases by 10 L and simultaneously the steam cools, losing 3,000 kJ of energy to the surroundings. What is the change in energy of the steam? (101.3 J  1 L atm)

The enthalpy of combustion of table sugar (sucrose, C₁₂H₂₂O₁₁, 342.3 g/mol) is 5,643 kJ/mol. What is the food value (Cal/g) of sucrose? (1 Cal  4.184 kJ)

A diver jumps off a diving board. At which point in the diagram below will the diver possess the greatest potential energy?

Assuming that the distances between the two ions are the same in all cases, which of the following ion pairs has the greatest electrostatic potential energy (i.e., largest in magnitude)?

According to Coulomb's law, which ionic compound A-D has the largest electrostatic potential energy (i.e., largest in magnitude)?

Suppose you eat a one-third pound hamburger without bread, cheese, or other items. Approximately how long would you need to walk to use up the calories in the hamburger? Assume the mass of the hamburger is 150 g with 3.6 Cal/g and that walking requires 2.5 times a basal metabolic rate of 280 kJ/hr.

Fuel density is ________

Which statement regarding combustion of a sample of gasoline in a bomb calorimeter is correct?

Given the following thermochemical equation detailing the combustion of glucose C₆H₁₂O₆(s) 6O₂(g) CO₂(g) 6H₂O(g) H_rxn 2803 kJ/mol C₆_H₁₂O₆ Determine the amount of glucose needed to release 30 kJ of energy.

How much work does a gas do when it expands against a constant pressure of 0.500 atm from a volume of 50.00 mL to a volume of 350.00 mL? (101.3 J  1 L atm)

The kinetic energy associated with the random motion of molecules is called ________

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

Exam 5: Thermochemistry: Energy Changes in Reactions

During a(n) ________ process, energy is transferred to the system from the surroundings.

Write the equation that corresponds to the standard enthalpy of formation for each of the following compounds: a) NaI(s), b) HClO4(g), and c) CH3OCH3(g)

A heating curve for some substance is shown below. Which of the line segments (I-V) represents heating of the liquid?

Determine the enthalpy for the following reaction, given  (NH3(g))  46.1 kJ/mol, (NO(g))  90.3 kJ/mol, and  (H2O(g))  241.8 kJ/mol. 4NH3(g) 5O2(g) 4NO(g) 6H2O(g) Hrxn  ? kJ

According to the first law of thermodynamics, which of the changes A-D will always increase the internal energy of a system? (q = energy transferred, and w = work done)

In a steam engine, steam in a cylinder expands against a piston, exerting 10 atm of external pressure. The volume of the cylinder increases by 10 L and simultaneously the steam cools, losing 3,000 kJ of energy to the surroundings. What is the change in energy of the steam? (101.3 J  1 L atm)

The enthalpy of combustion of table sugar (sucrose, C12H22O11, 342.3 g/mol) is 5,643 kJ/mol. What is the food value (Cal/g) of sucrose? (1 Cal  4.184 kJ)

A diver jumps off a diving board. At which point in the diagram below will the diver possess the greatest potential energy?

Assuming that the distances between the two ions are the same in all cases, which of the following ion pairs has the greatest electrostatic potential energy (i.e., largest in magnitude)?

According to Coulomb's law, which ionic compound A-D has the largest electrostatic potential energy (i.e., largest in magnitude)?

Suppose you eat a one-third pound hamburger without bread, cheese, or other items. Approximately how long would you need to walk to use up the calories in the hamburger? Assume the mass of the hamburger is 150 g with 3.6 Cal/g and that walking requires 2.5 times a basal metabolic rate of 280 kJ/hr.

Fuel density is ________

Which statement regarding combustion of a sample of gasoline in a bomb calorimeter is correct?

Given the following thermochemical equation detailing the combustion of glucose C6H12O6(s) 6O2(g) CO2(g) 6H2O(g) Hrxn  2803 kJ/mol C6H12O6 Determine the amount of glucose needed to release 30 kJ of energy.

How much work does a gas do when it expands against a constant pressure of 0.500 atm from a volume of 50.00 mL to a volume of 350.00 mL? (101.3 J  1 L atm)

The kinetic energy associated with the random motion of molecules is called ________

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

Write the equation that corresponds to the standard enthalpy of formation for each of the following compounds: a) NaI(s), b) HClO₄(g), and c) CH₃OCH₃(g)

Determine the enthalpy for the following reaction, given  (NH₃(g))  46.1 kJ/mol, (NO(g))  90.3 kJ/mol, and  (H₂O(g))  241.8 kJ/mol. 4NH₃(g) 5O₂(g) 4NO(g) 6H₂O(g) H_rxn  ? kJ

The enthalpy of combustion of table sugar (sucrose, C₁₂H₂₂O₁₁, 342.3 g/mol) is 5,643 kJ/mol. What is the food value (Cal/g) of sucrose? (1 Cal  4.184 kJ)

Given the following thermochemical equation detailing the combustion of glucose C₆H₁₂O₆(s) 6O₂(g) CO₂(g) 6H₂O(g) H_rxn 2803 kJ/mol C₆_H₁₂O₆ Determine the amount of glucose needed to release 30 kJ of energy.