Thermochemistry Calculations Practice Test
Calculation Type I: Specific Heat Capacity - (𝑄 = 𝑚𝑐∆𝑇)
1. Calculate the heat (Q) in Joules absorbed by 15.0 g of liquid water to raise its temperature from 20.0°C
to 50.0°C. (c_water = 4.18 J/g°C)
2. Determine the energy in Joules required to heat a 45.0 g block of aluminum from 25.0°C to 75.0°C.
(c_Al = 0.897 J/g°C)
3. A 1.20 kg sample of water is heated from 10.0°C to 90.0°C. Calculate the total heat absorbed in
kilojoules (kJ).
4. How much energy is transferred to a 25.0 g block of lead to increase its temperature by 15.0°C?
(c_lead = 0.128 J/g°C)
5. Calculate the heat released (in Joules) when a 500.0 g copper pipe cools from 100.0°C to 20.0°C. (c_Cu
= 0.385 J/g°C)
6. A 5.00 g piece of iron (c = 0.449 J/g°C) transfers 180. J of heat. Calculate the total change in
temperature (ΔT).
7. A 121.6 g sample of lead (c = 0.128 J/g°C) is initially at 20.4°C. If it absorbs 450. J of energy, calculate
the final temperature (T_f).
8. If a 50.0 g sample of water at 25.0°C absorbs 2090 J of heat, what is the resulting final temperature?
9. A 200.0 g block of silver (c = 0.235 J/g°C) at 150.0°C loses 2350 J of heat. Calculate its final
temperature.
10. How many grams of water are present if 15,048 J of energy are required to increase the temperature
from 25.0°C to 55.0°C?
11. Determine the mass of an iron block (c = 0.449 J/g°C) that releases 500. J of heat when cooling by
20.0°C.
12. A lead weight undergoes a temperature increase of 12.0°C after absorbing 153.6 J. Calculate the
mass of the lead.
13. A 121.6 g sample of an unknown metal rose from 20.4°C to 35.5°C when 235 J of heat were added.
Calculate the specific heat capacity (c) and identify the metal using the lead constant (c = 0.128 J/g°C).
14. A 20.0 g sample of an unknown substance absorbs 418 J to increase its temperature by 5.0°C.
Calculate the specific heat capacity.
15. A 35.0 g sample of an unknown metal at 98.0°C is placed in a calorimeter and cools to 22.0°C,
releasing 1066.1 J. Calculate its specific heat capacity.
, Thermochemistry Calculations Practice Test
Calculation Type II: Heat Capacity of Systems - (𝑄 = 𝑐∆𝑇)
1. A calorimeter with a known heat capacity of 1.258 kJ/°C undergoes a temperature rise of 13.7°C. How
much heat (Q) did the calorimeter absorb?
2. During a reaction, a calorimeter (C = 9.63 kJ/°C) showed a temperature increase of 8.7°C. Calculate the
heat absorbed in kJ.
3. A solution calorimeter with a heat capacity of 1071 J/°C recorded a temperature drop of 3.44°C.
Calculate the heat change in Joules.
4. If a bomb calorimeter has a heat capacity of 12.05 kJ/°C and its temperature rises by 12.2°C, how
much energy was released into the system?
5. A system has a heat capacity of 547 J/°C. If the temperature increases from 25.0°C to 36.7°C, calculate
the total heat (Q) absorbed.
6. A calorimeter (C = 13.72 kJ/°C) experiences a temperature drop of 7.00°C. Calculate the energy change
in kJ.
7. Calculate the heat released by a system (C = 1.50 kJ/°C) when the temperature rises by 5.5°C.
8. A reaction with Cl2 released 96.04 kJ of energy into a calorimeter, causing the temperature to rise by
exactly 7.00°C. Calculate the ΔH for using 2 moles of 23.2 g of Cl2.
9. An experimental trial releases 17,234 J of energy, causing a calorimeter's temperature to rise by
13.7°C. Determine the system heat capacity in J/°C.
10. A combustion reaction with 12.9 g of HBr in a bomb calorimeter releases 83.78 kJ. The temperature
rises by 8.7°C. What is the heat involved per 1.0 mol of HBr used in this reaction?
11. A 147.01 kJ energy release results in a 12.2°C temperature increase in a calorimeter. Calculate its
heat capacity in kJ/°C.
12. When 6399.9 J of energy is absorbed by a system, the temperature rises by 11.7°C. Calculate the heat
capacity in J/°C.
13. A reaction causes a temperature decrease of 3.44°C in a system. If the total heat change was
measured at 3684 J, what is the heat capacity?
14. A specialized container undergoes a 5.00°C change when 25.0 kJ of heat is added. Calculate C in
kJ/°C.
15. If 500. J of energy causes a 2.5°C rise in a Dewar flask, what is the flask's heat capacity in J/°C?
Calculation Type I: Specific Heat Capacity - (𝑄 = 𝑚𝑐∆𝑇)
1. Calculate the heat (Q) in Joules absorbed by 15.0 g of liquid water to raise its temperature from 20.0°C
to 50.0°C. (c_water = 4.18 J/g°C)
2. Determine the energy in Joules required to heat a 45.0 g block of aluminum from 25.0°C to 75.0°C.
(c_Al = 0.897 J/g°C)
3. A 1.20 kg sample of water is heated from 10.0°C to 90.0°C. Calculate the total heat absorbed in
kilojoules (kJ).
4. How much energy is transferred to a 25.0 g block of lead to increase its temperature by 15.0°C?
(c_lead = 0.128 J/g°C)
5. Calculate the heat released (in Joules) when a 500.0 g copper pipe cools from 100.0°C to 20.0°C. (c_Cu
= 0.385 J/g°C)
6. A 5.00 g piece of iron (c = 0.449 J/g°C) transfers 180. J of heat. Calculate the total change in
temperature (ΔT).
7. A 121.6 g sample of lead (c = 0.128 J/g°C) is initially at 20.4°C. If it absorbs 450. J of energy, calculate
the final temperature (T_f).
8. If a 50.0 g sample of water at 25.0°C absorbs 2090 J of heat, what is the resulting final temperature?
9. A 200.0 g block of silver (c = 0.235 J/g°C) at 150.0°C loses 2350 J of heat. Calculate its final
temperature.
10. How many grams of water are present if 15,048 J of energy are required to increase the temperature
from 25.0°C to 55.0°C?
11. Determine the mass of an iron block (c = 0.449 J/g°C) that releases 500. J of heat when cooling by
20.0°C.
12. A lead weight undergoes a temperature increase of 12.0°C after absorbing 153.6 J. Calculate the
mass of the lead.
13. A 121.6 g sample of an unknown metal rose from 20.4°C to 35.5°C when 235 J of heat were added.
Calculate the specific heat capacity (c) and identify the metal using the lead constant (c = 0.128 J/g°C).
14. A 20.0 g sample of an unknown substance absorbs 418 J to increase its temperature by 5.0°C.
Calculate the specific heat capacity.
15. A 35.0 g sample of an unknown metal at 98.0°C is placed in a calorimeter and cools to 22.0°C,
releasing 1066.1 J. Calculate its specific heat capacity.
, Thermochemistry Calculations Practice Test
Calculation Type II: Heat Capacity of Systems - (𝑄 = 𝑐∆𝑇)
1. A calorimeter with a known heat capacity of 1.258 kJ/°C undergoes a temperature rise of 13.7°C. How
much heat (Q) did the calorimeter absorb?
2. During a reaction, a calorimeter (C = 9.63 kJ/°C) showed a temperature increase of 8.7°C. Calculate the
heat absorbed in kJ.
3. A solution calorimeter with a heat capacity of 1071 J/°C recorded a temperature drop of 3.44°C.
Calculate the heat change in Joules.
4. If a bomb calorimeter has a heat capacity of 12.05 kJ/°C and its temperature rises by 12.2°C, how
much energy was released into the system?
5. A system has a heat capacity of 547 J/°C. If the temperature increases from 25.0°C to 36.7°C, calculate
the total heat (Q) absorbed.
6. A calorimeter (C = 13.72 kJ/°C) experiences a temperature drop of 7.00°C. Calculate the energy change
in kJ.
7. Calculate the heat released by a system (C = 1.50 kJ/°C) when the temperature rises by 5.5°C.
8. A reaction with Cl2 released 96.04 kJ of energy into a calorimeter, causing the temperature to rise by
exactly 7.00°C. Calculate the ΔH for using 2 moles of 23.2 g of Cl2.
9. An experimental trial releases 17,234 J of energy, causing a calorimeter's temperature to rise by
13.7°C. Determine the system heat capacity in J/°C.
10. A combustion reaction with 12.9 g of HBr in a bomb calorimeter releases 83.78 kJ. The temperature
rises by 8.7°C. What is the heat involved per 1.0 mol of HBr used in this reaction?
11. A 147.01 kJ energy release results in a 12.2°C temperature increase in a calorimeter. Calculate its
heat capacity in kJ/°C.
12. When 6399.9 J of energy is absorbed by a system, the temperature rises by 11.7°C. Calculate the heat
capacity in J/°C.
13. A reaction causes a temperature decrease of 3.44°C in a system. If the total heat change was
measured at 3684 J, what is the heat capacity?
14. A specialized container undergoes a 5.00°C change when 25.0 kJ of heat is added. Calculate C in
kJ/°C.
15. If 500. J of energy causes a 2.5°C rise in a Dewar flask, what is the flask's heat capacity in J/°C?
