Chem 1441 Test Questions from Previous Exams Page 1 of 7
Test 3 – Chapters 6 and 7 (Rogers Textbook)
Chapter 6 – Thermochemistry
1. Which of the following properties is not a state function?
a) temperature
b) enthalpy
c) work
d) volume
e) internal energy
2. What is the kinetic energy of a 45 g golf ball moving at 61 m/s?
a) 1.4 J
b) 2700 J
c) 1400 J
d) 84 J
e) 84,000 J
3. Which one of the following will have a greater kinetic energy?
a) a 10 kg object traveling at 5 m/s
b) a 5 kg object traveling at 10 m/s
c) both of these have the same kinetic energy
4. Suppose that an endothermic chemical reaction occurs inside of an insulated container that allows no heat to enter or leave the
system. Which statement below is true?
a) The temperature of the contents of the container decreases.
b) The temperature of the contents of the container increases.
c) The temperature of the contents of the container does not change.
d) The temperature of the surroundings around the container decreases.
e) Choices (b) and (d) are both correct.
5. Which of the following processes is endothermic?
a) 2H2(g) + O2(g) 2H2O(g)
b) H2O(g) H2O(l)
c) CH4(g) + 2O2(g) CO2(g) + 2H2O(l)
d) H2O(s) H2O(l)
e) None of these.
6. Which of the following processes is exothermic?
a) ice melting
b) water evaporating
c) Ammonium thiocyanate and barium hydroxide are mixed at 25°C. When they react, the temperature drops.
d) sublimation of dry ice (solid CO2)
e) condensation of water vapor
7. The heat gained or lost by the contents of a bomb calorimeter is equal to:
a) ∆H
b) ∆E
c) w
d) ∆H + P∆V
e) qP
8. For a process at constant pressure,
a) ∆E = w and q = 0
b) ∆E = q and w = 0
c) ∆E = ∆H
d) ∆H = q
e) choices b and c are both correct
, Chem 1441 Test Questions from Previous Exams Page 2 of 7
Test 3 – Chapters 6 and 7 (Rogers Textbook)
9. What is the value of ∆E for a system that performs 213 kJ of work on its surroundings and loses 79 kJ of heat?
a) +292 kJ
b) -292 kJ
c) +134 kJ
d) -134 kJ
e) -213 kJ
10. A certain reaction was performed under a constant pressure of 15.0 atm. During the reaction, the volume contracted from 10.75 L
to 3.68 L, and 7.33 kJ of heat was given off. What is ∆E for this reaction?
a) +3.38 kJ
b) -18.0 kJ
c) +98.7 kJ
d) +10.7 kJ
e) -113 kJ
11. Consider the following thermochemical equation:
2Na2O2(s) + 2H2O(l) 4NaOH(s) + O2(g) ∆H° = -126 kJ
How much heat would be evolved by the reaction of 25.0 g of Na 2O2 with water?
a) 10.1 kJ
b) 20.2 kJ
c) 40.4 kJ
d) 67.5 kJ
e) 80.8 kJ
12. The specific heat of copper metal is 0.385 J/g.°C. How many joules of heat are required to raise the temperature of a 1.42 kg
block of copper from 25.0°C to 88.5 °C?
a) 34.7 J
b) 48.4 J
c) 62.1 J
d) 3.47 x 104 J
e) 6.21 x 103 J
13. Consider two samples A and B of the same substance which are at the same temperature in separate containers from which no
heat can escape. Sample A has a greater mass than sample B. Equal amounts of heat are added to each sample. What happens?
a) Both samples increase in temperature by the same amount.
b) The specific heat of the substance will be different in the two samples.
c) The temperature of sample A rises more than the temperature of sample B.
d) The temperature of sample B rises more than the temperature of sample A.
e) The change in temperature of the two samples depends on their relative densities.
14. 60.0 g of iron, 80.0 g of copper, and 50.0 g of aluminum were each initially at 25°C. If each of these substances gained 100 J of
heat, which would have the highest temperature?
a) 60.0 g of Fe (specific heat of Fe = 0.450 J/g.°C)
b) 50.0 g of Al (specific heat of Al = 0.902 J/g.°C)
c) 80.0 g of Cu (specific heat of Cu = 0.385 J/g.°C)
d) All three substances would have the same temperature.
e) There is no way to determine.
15. A 275 g sample of nickel at 100.0ºC is placed in 100.0 mL of water at 22.0ºC. What is the final temperature of the mixture,
assuming no heat is lost to the surroundings? The specific heat capacity of Ni is 0.444 J/(g .K). The density of water is 1.00
g/mL and the specific heat capacity of water is 4.18 J/(g.K).
a) 39.6ºC
b) 40.8ºC
c) 61.0ºC
d) 79.2ºC
e) 82.4ºC
Test 3 – Chapters 6 and 7 (Rogers Textbook)
Chapter 6 – Thermochemistry
1. Which of the following properties is not a state function?
a) temperature
b) enthalpy
c) work
d) volume
e) internal energy
2. What is the kinetic energy of a 45 g golf ball moving at 61 m/s?
a) 1.4 J
b) 2700 J
c) 1400 J
d) 84 J
e) 84,000 J
3. Which one of the following will have a greater kinetic energy?
a) a 10 kg object traveling at 5 m/s
b) a 5 kg object traveling at 10 m/s
c) both of these have the same kinetic energy
4. Suppose that an endothermic chemical reaction occurs inside of an insulated container that allows no heat to enter or leave the
system. Which statement below is true?
a) The temperature of the contents of the container decreases.
b) The temperature of the contents of the container increases.
c) The temperature of the contents of the container does not change.
d) The temperature of the surroundings around the container decreases.
e) Choices (b) and (d) are both correct.
5. Which of the following processes is endothermic?
a) 2H2(g) + O2(g) 2H2O(g)
b) H2O(g) H2O(l)
c) CH4(g) + 2O2(g) CO2(g) + 2H2O(l)
d) H2O(s) H2O(l)
e) None of these.
6. Which of the following processes is exothermic?
a) ice melting
b) water evaporating
c) Ammonium thiocyanate and barium hydroxide are mixed at 25°C. When they react, the temperature drops.
d) sublimation of dry ice (solid CO2)
e) condensation of water vapor
7. The heat gained or lost by the contents of a bomb calorimeter is equal to:
a) ∆H
b) ∆E
c) w
d) ∆H + P∆V
e) qP
8. For a process at constant pressure,
a) ∆E = w and q = 0
b) ∆E = q and w = 0
c) ∆E = ∆H
d) ∆H = q
e) choices b and c are both correct
, Chem 1441 Test Questions from Previous Exams Page 2 of 7
Test 3 – Chapters 6 and 7 (Rogers Textbook)
9. What is the value of ∆E for a system that performs 213 kJ of work on its surroundings and loses 79 kJ of heat?
a) +292 kJ
b) -292 kJ
c) +134 kJ
d) -134 kJ
e) -213 kJ
10. A certain reaction was performed under a constant pressure of 15.0 atm. During the reaction, the volume contracted from 10.75 L
to 3.68 L, and 7.33 kJ of heat was given off. What is ∆E for this reaction?
a) +3.38 kJ
b) -18.0 kJ
c) +98.7 kJ
d) +10.7 kJ
e) -113 kJ
11. Consider the following thermochemical equation:
2Na2O2(s) + 2H2O(l) 4NaOH(s) + O2(g) ∆H° = -126 kJ
How much heat would be evolved by the reaction of 25.0 g of Na 2O2 with water?
a) 10.1 kJ
b) 20.2 kJ
c) 40.4 kJ
d) 67.5 kJ
e) 80.8 kJ
12. The specific heat of copper metal is 0.385 J/g.°C. How many joules of heat are required to raise the temperature of a 1.42 kg
block of copper from 25.0°C to 88.5 °C?
a) 34.7 J
b) 48.4 J
c) 62.1 J
d) 3.47 x 104 J
e) 6.21 x 103 J
13. Consider two samples A and B of the same substance which are at the same temperature in separate containers from which no
heat can escape. Sample A has a greater mass than sample B. Equal amounts of heat are added to each sample. What happens?
a) Both samples increase in temperature by the same amount.
b) The specific heat of the substance will be different in the two samples.
c) The temperature of sample A rises more than the temperature of sample B.
d) The temperature of sample B rises more than the temperature of sample A.
e) The change in temperature of the two samples depends on their relative densities.
14. 60.0 g of iron, 80.0 g of copper, and 50.0 g of aluminum were each initially at 25°C. If each of these substances gained 100 J of
heat, which would have the highest temperature?
a) 60.0 g of Fe (specific heat of Fe = 0.450 J/g.°C)
b) 50.0 g of Al (specific heat of Al = 0.902 J/g.°C)
c) 80.0 g of Cu (specific heat of Cu = 0.385 J/g.°C)
d) All three substances would have the same temperature.
e) There is no way to determine.
15. A 275 g sample of nickel at 100.0ºC is placed in 100.0 mL of water at 22.0ºC. What is the final temperature of the mixture,
assuming no heat is lost to the surroundings? The specific heat capacity of Ni is 0.444 J/(g .K). The density of water is 1.00
g/mL and the specific heat capacity of water is 4.18 J/(g.K).
a) 39.6ºC
b) 40.8ºC
c) 61.0ºC
d) 79.2ºC
e) 82.4ºC
