Question 1

Which one of the following relationships is always correct?

Accepted Answer

A)  potential energy + kinetic energy = constant
B)  E = q + w
C)  Δ E = Δ H − PΔ V
D)  H = E + PV
E)  Δ H = q vF) B) and D)
G) A) and D)

Question 2

When Karl Kaveman adds chilled grog to his new granite mug, he removes 10.9 kJ of energy from the mug. If it has a mass of 625 g and was at 25°C, what is its new temperature? Specific heat capacity of granite = 0.79 J/(g·K)

Accepted Answer

A)  3°C
B)  14°C
C)  22°C
D)  47°C
E)  None of these choices are correct.F) A) and C)
G) B) and E)

Question 3

What is the final temperature when 20.0 g of water at 25°C is mixed with 30.0 g of water at 80°C?

Accepted Answer

A)  35°C
B)  42°C
C)  53°C
D)  58°C
E)  70°CF) C) and E)
G) All of the above D

Question 4

In which one of the following processes is ΔH = ΔE?

Accepted Answer

A)  2HI(g) → H 2(g) + I 2(g) at atmospheric pressure.
B)  Two moles of ammonia gas are cooled from 325 °C to 300 °C at 1.2 atm.
C)  H 2O(l) → H 2O(g) at 100 °C at atmospheric pressure.
D)  CaCO 3(s) → CaO(s) + CO 2(g) at 800 °C at atmospheric pressure.
E)  CO 2(s) → CO 2(g) at atmospheric pressure.F) B) and D)
G) A) and B) A

Question 5

40.0 g of ice cubes at 0.0°C are combined with 150 g of liquid water at 20.0°C in a coffee cup calorimeter. Calculate the final temperature reached, assuming no heat loss or gain from the surroundings. (Data: specific heat capacity of H2O(l) , c = 4.18 J/g·°C; H2O(s)  → H2O(l)  ΔH = 6.02 kJ/mol)

Accepted Answer

A)  0.0
B)  10.6
C)  30.7
D)  43.2
E)  56.4F) A) and B)
G) None of the above

Question 6

A 275-g sample of nickel at 100.0°C is placed in 100.0 mL of water at 22.0°C. What is the final temperature of the water? Assume that no heat is lost to or gained from the surroundings. Specific heat capacity of nickel = 0.444 J/(g·K)

Accepted Answer

A)  39.6°C
B)  40.8°C
C)  61.0°C
D)  79.2°C
E)  82.4°CF) B) and E)
G) C) and D)

Question 7

Calculate the enthalpy change for the reaction NO(g)  + O(g)  → NO2(g) 
From the following data:
NO(g)  + O3(g)  → NO2(g)  + O2(g)  ΔH = −198.9 kJ
O3(g)  → 1.5O2(g)  ΔH = −142.3 kJ
O2(g)  → 2O(g)  ΔH = 495.0 kJ

Accepted Answer

A)  −551.6 kJ
B)  −304.1 kJ
C)  190.9 kJ
D)  153.8 kJ
E)  438.4 kJF) A) and D)
G) A) and C)

Question 8

The specific heat capacity c of a metal is approximately related to its molar massℳ as follows: c ×ℳ = 3R, where R is the universal gas constant, 8.314 J/mol·K. Use this relationship to identify the metal which has a specific heat capacity of 0.900 J/g·K.

Accepted Answer

A)  Li
B)  Sn
C)  Ca
D)  Al
E)  UF) B) and E)
G) None of the above

Question 9

For a reaction in a sealed, rigid container, ΔH is always greater than ΔE.

Accepted Answer

A) True 
 B)False

Question 10

A system that undergoes an adiabatic change and has work done on it by the surroundings has

Accepted Answer

A)  w = Δ E.
B)  w = −Δ E.
C)  w > 0, Δ E 
D)  w  0.
E)  w > Δ E.F) A) and B)
G) B) and D)

Question 11

ΔE values obtained by bomb calorimetry can be converted to give accurate ΔH values.

Accepted Answer

A) True 
 B)False

Question 12

A 1.00 g piece of copper metal is initially at 100.0°C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20.0°C. After stirring, the final temperature of both copper and water is 25.0°C. Assuming no heat losses, and that the specific heat (capacity)  of water is 4.18 J/(g·K) , what is the heat capacity of the copper in J/K?

Accepted Answer

A)  2.79 J/(g·K) 
B)  3.33 J/(g·K) 
C)  13.9 J/(g·K) 
D)  209 J/(g·K) 
E)  None of these choices are correct.F) None of the above
G) B) and C)

Question 13

For all processes, both q and w will have the same sign.

Accepted Answer

A) True 
 B)False

Question 14

A backpacker collects snow at 0°C, and places it in a cooking pot on a camp stove. It takes 643 kJ of heat energy to melt the snow and bring the water to boiling. Assuming no heat loss, and neglecting the specific heat capacity of the pot, calculate the mass of snow that the backpacker collected. (Data: specific heat capacity of liquid water, c = 4.18 J/g·K; and: H2O(s)  → H2O(l)  ΔH = ΔHfusion = 6.02 kJ/mol)

Accepted Answer

A)  1.92 kg
B)  1.90 kg
C)  1.52 kg
D)  855 g
E)  < 800 gF) A) and B)
G) A) and E) D

Question 15

A common laboratory reaction is the neutralization of an acid with a base. When 50.0 mL of 0.500 M HCl at 25.0°C is added to 50.0 mL of 0.500 M NaOH at 25.0°C in a coffee cup calorimeter, the temperature of the mixture rises to 28.2°C. What is the heat of reaction per mole of acid? Assume the mixture has a specific heat capacity of 4.18 J/(g·K)  and that the densities of the reactant solutions are both 1.00 g/mL.

Accepted Answer

A)  670 J
B)  1300 J
C)  27 kJ
D)  54 kJ
E)  > 100 kJF) A) and C)
G) All of the above

Question 16

An ideal gas (the system)  is contained in a flexible balloon at a pressure of 1 atm and is initially at a temperature of 20°C. The surrounding air is at the same pressure, but its temperature is 25°C. When the system has equilibrated with its surroundings, both systems and surroundings are at 25°C and 1 atm. In changing from the initial to the final state, which one of the following relationships regarding the system is correct?

Accepted Answer

A)  Δ E 
B)  Δ E = 0
C)  Δ H = 0
D)  w > 0
E)  q > 0F) B) and E)
G) D) and E)

Question 17

In a reaction with high energy reactants and low energy products, q is negative.

Accepted Answer

A) True 
 B)False

Question 18

The enthalpy (H) of liquid water is greater than that of the same quantity of ice at the same temperature.

Accepted Answer

A) True 
 B)False

Question 19

Which one of the following is a correct formation reaction?

Accepted Answer

A)  C(diamond) → C(graphite) 
B)  H 2( g) + O( g) → H 2O( l) 
C)  C(graphite) + 4H( g) → CH 4( g) 
D)  6C(graphite) + 6H 2O( s) → C 6H 12O 6( s) 
E)  2C(graphite) + 3H 2( g) + ½O 2( g) → C 2H 5OH( l) F) A) and E)
G) A) and D)

Question 20

Natural gas, or methane, is an important fuel. Combustion of one mole of methane releases 802.3 kilojoules of energy. How much energy does that represent in kilocalories?

Accepted Answer

A)  1.92 × 10 −1 kcal
B)  1.92 × 10 2 kcal
C)  3.36 × 10 3 kcal
D)  1.92 × 10 5 kcal
E)  3.36 × 10 6 kcalF) A) and B)
G) All of the above

Exam 6: Thermochemistry: Energy Flow and Chemical Change

Which one of the following relationships is always correct?

Correct Answer
verified

When Karl Kaveman adds chilled grog to his new granite mug, he removes 10.9 kJ of energy from the mug. If it has a mass of 625 g and was at 25°C, what is its new temperature? Specific heat capacity of granite = 0.79 J/(g·K)

Correct Answer
verified

What is the final temperature when 20.0 g of water at 25°C is mixed with 30.0 g of water at 80°C?

Correct Answer
verified
D

In which one of the following processes is ΔH = ΔE?

Correct Answer
verified
A

Correct Answer
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A 275-g sample of nickel at 100.0°C is placed in 100.0 mL of water at 22.0°C. What is the final temperature of the water? Assume that no heat is lost to or gained from the surroundings. Specific heat capacity of nickel = 0.444 J/(g·K)

Correct Answer
verified

Calculate the enthalpy change for the reaction NO(g) + O(g) → NO₂(g) From the following data: NO(g) + O₃(g) → NO₂(g) + O₂(g) ΔH = −198.9 kJ O₃(g) → 1.5O₂(g) ΔH = −142.3 kJ O₂(g) → 2O(g) ΔH = 495.0 kJ

Correct Answer
verified

The specific heat capacity c of a metal is approximately related to its molar massℳ as follows: c ×ℳ = 3R, where R is the universal gas constant, 8.314 J/mol·K. Use this relationship to identify the metal which has a specific heat capacity of 0.900 J/g·K.

Correct Answer
verified

For a reaction in a sealed, rigid container, ΔH is always greater than ΔE.

Correct Answer
verified

A system that undergoes an adiabatic change and has work done on it by the surroundings has

Correct Answer
verified

ΔE values obtained by bomb calorimetry can be converted to give accurate ΔH values.

Correct Answer
verified

Correct Answer
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For all processes, both q and w will have the same sign.

Correct Answer
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Correct Answer
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D

Correct Answer
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Correct Answer
verified

In a reaction with high energy reactants and low energy products, q is negative.

Correct Answer
verified

The enthalpy (H) of liquid water is greater than that of the same quantity of ice at the same temperature.

Correct Answer
verified

Which one of the following is a correct formation reaction?

Correct Answer
verified

Natural gas, or methane, is an important fuel. Combustion of one mole of methane releases 802.3 kilojoules of energy. How much energy does that represent in kilocalories?

Correct Answer
verified

Exam 6: Thermochemistry: Energy Flow and Chemical Change

Which one of the following relationships is always correct?

Correct AnswerverifiedShow Answer

When Karl Kaveman adds chilled grog to his new granite mug, he removes 10.9 kJ of energy from the mug. If it has a mass of 625 g and was at 25°C, what is its new temperature? Specific heat capacity of granite = 0.79 J/(g·K)

Correct AnswerverifiedShow Answer

What is the final temperature when 20.0 g of water at 25°C is mixed with 30.0 g of water at 80°C?

Correct AnswerverifiedD

In which one of the following processes is ΔH = ΔE?

Correct AnswerverifiedA

Correct AnswerverifiedShow Answer

A 275-g sample of nickel at 100.0°C is placed in 100.0 mL of water at 22.0°C. What is the final temperature of the water? Assume that no heat is lost to or gained from the surroundings. Specific heat capacity of nickel = 0.444 J/(g·K)

Correct AnswerverifiedShow Answer

Calculate the enthalpy change for the reaction NO(g) + O(g) → NO2(g) From the following data: NO(g) + O3(g) → NO2(g) + O2(g) ΔH = −198.9 kJ O3(g) → 1.5O2(g) ΔH = −142.3 kJ O2(g) → 2O(g) ΔH = 495.0 kJ

Correct AnswerverifiedShow Answer

The specific heat capacity c of a metal is approximately related to its molar massℳ as follows: c ×ℳ = 3R, where R is the universal gas constant, 8.314 J/mol·K. Use this relationship to identify the metal which has a specific heat capacity of 0.900 J/g·K.

Correct AnswerverifiedShow Answer

For a reaction in a sealed, rigid container, ΔH is always greater than ΔE.

Correct AnswerverifiedShow Answer

A system that undergoes an adiabatic change and has work done on it by the surroundings has

Correct AnswerverifiedShow Answer

ΔE values obtained by bomb calorimetry can be converted to give accurate ΔH values.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

For all processes, both q and w will have the same sign.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedD

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

In a reaction with high energy reactants and low energy products, q is negative.

Correct AnswerverifiedShow Answer

The enthalpy (H) of liquid water is greater than that of the same quantity of ice at the same temperature.

Correct AnswerverifiedShow Answer

Which one of the following is a correct formation reaction?

Correct AnswerverifiedShow Answer

Natural gas, or methane, is an important fuel. Combustion of one mole of methane releases 802.3 kilojoules of energy. How much energy does that represent in kilocalories?

Correct AnswerverifiedShow Answer

Correct Answer
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D

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A

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Calculate the enthalpy change for the reaction NO(g) + O(g) → NO₂(g) From the following data: NO(g) + O₃(g) → NO₂(g) + O₂(g) ΔH = −198.9 kJ O₃(g) → 1.5O₂(g) ΔH = −142.3 kJ O₂(g) → 2O(g) ΔH = 495.0 kJ

Correct Answer
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D

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