AP Chemistry Practice Quiz: Heat Capacity and Calorimetry

Written by AP Content Team, Verified for 2026 AP Exams, Last updated: May 2026

Test your understanding with short quizzes. This quiz has 15 questions to check your progress.

Question 1 of 15

According to the provided information, which equation is used to quantify the amount of heat transferred during the heating or cooling of a substance?

A)q = m/ΔTB)q = mcΔTC)q = cΔT/mD)q = m + c + ΔT

All Questions (15)

According to the provided information, which equation is used to quantify the amount of heat transferred during the heating or cooling of a substance?

A) q = m/ΔT

B) q = mcΔT

C) q = cΔT/m

D) q = m + c + ΔT

Correct Answer: B

The content explicitly states that the amount of heat transferred is quantified by the equation q = mcΔT, where q is heat, m is mass, c is specific heat capacity, and ΔT is the change in temperature.

Two equal masses of different substances, Substance X and Substance Y, absorb the same amount of thermal energy. If Substance X has a higher specific heat capacity than Substance Y, what can be concluded about their temperature changes?

A) Substance X will have a greater temperature change than Substance Y.

B) Substance Y will have a greater temperature change than Substance X.

C) Both substances will have the same temperature change.

D) The temperature change cannot be determined without knowing the molar heat capacity.

Correct Answer: B

The content states that the transfer of a given amount of thermal energy will not produce the same temperature change in equal masses of matter with differing specific heat capacities. Since q and m are the same for both, and q = mcΔT, the substance with the lower specific heat capacity (Substance Y) must have a larger temperature change (ΔT) to balance the equation.

In a calorimetry experiment, a salt is dissolved in water, and the temperature of the resulting mixture is observed to decrease. This observation indicates that the dissolution process is:

A) Exothermic, releasing heat into the surroundings.

B) Endothermic, absorbing heat from the surroundings.

C) Thermally neutral, with no heat exchange.

D) A phase transition, not a chemical process.

Correct Answer: B

The provided text states that in calorimetry experiments for dissolution, a decrease in mixture temperature indicates an endothermic process. The process absorbs heat from the water, causing the water's temperature to drop.

A hot piece of metal is placed into a container of cool water in an insulated system. Heat flows from the metal to the water until they reach thermal equilibrium. This process is a direct illustration of which fundamental principle?

A) The definition of molar heat capacity.

B) The first law of thermodynamics.

C) The process of endothermic dissolution.

D) The conditions required for a phase transition.

Correct Answer: B

The first law of thermodynamics states that energy is conserved. In this isolated system, the heat energy lost by the hot metal is gained by the cool water. This transfer and conservation of energy is a core concept of the first law.

When a chemical system is cooled, what is the effect on the energy of the system?

A) The energy of the system increases.

B) The energy of the system decreases.

C) The energy of the system remains constant.

D) The energy of the system is converted into mass.

Correct Answer: B

The content explicitly states that 'cooling a system decreases the energy of the system.' This is because heat, a form of energy, is being removed from the system.

Which of the following is NOT listed as one of the three main processes through which chemical systems change their energy?

A) Heating/cooling

B) Phase transitions

C) Chemical reactions

D) Changes in pressure

Correct Answer: D

The provided content identifies three main processes for energy change in chemical systems: heating/cooling, phase transitions, and chemical reactions. Changes in pressure, while related to energy in thermodynamics (work), is not listed as one of these three main processes in the given text.

A chemist needs to calculate the heat absorbed by a sample of water. Besides the initial and final temperatures, what two quantities are necessary if they plan to use the specific heat capacity of water?

A) The mass of the water and its specific heat capacity.

B) The volume of the water and its molar heat capacity.

C) The number of moles of water and its density.

D) The mass of the water and its molar heat capacity.

Correct Answer: A

The equation q = mcΔT is used for this calculation. To find q (heat), one needs m (mass), c (specific heat capacity), and ΔT (change in temperature). Since ΔT is already known, the mass and specific heat capacity are the required quantities.

If a calorimetry experiment for the dissolution of a compound shows a significant increase in the temperature of the water, what can be inferred about the process based on the first law of thermodynamics?

A) The process is endothermic, and the system created energy.

B) The process is exothermic, and energy was transferred from the chemical system to the water.

C) The process is endothermic, and energy was transferred from the water to the chemical system.

D) The process is exothermic, and the first law of thermodynamics does not apply to dissolution.

Correct Answer: B

An increase in temperature indicates an exothermic process. According to the first law, energy is conserved. Therefore, the energy that heated the water must have been released by the chemical system (the dissolving compound), transferring from the system to the surroundings (the water).

Both specific heat capacity and molar heat capacity are used in energy calculations. What is the fundamental difference in the 'amount of substance' unit used for each?

A) Specific heat capacity uses volume, while molar heat capacity uses mass.

B) Specific heat capacity uses mass, while molar heat capacity uses moles.

C) Specific heat capacity uses moles, while molar heat capacity uses mass.

D) Both use mass, but molar heat capacity is only for gases.

Correct Answer: B

The names themselves indicate the units. Specific heat capacity is the heat required to raise the temperature of a specific mass (typically one gram) by one degree. Molar heat capacity is the heat required to raise the temperature of one mole of a substance by one degree.

A student heats 100 g of a substance, and its temperature increases by 20°C. If the student repeats the experiment with 200 g of the same substance and adds the exact same amount of heat, what will be the approximate temperature change?

A) 40°C

B) 20°C

C) 10°C

D) 5°C

Correct Answer: C

Based on the equation q = mcΔT, the temperature change (ΔT) is inversely proportional to the mass (m) when heat (q) and specific heat capacity (c) are constant (ΔT = q/mc). If the mass is doubled from 100 g to 200 g, the temperature change will be halved, from 20°C to 10°C.

The measurement of heat transfer during physical or chemical processes is the central purpose of which experimental technique mentioned in the text?

A) Thermodynamics

B) Titration

C) Calorimetry

D) Spectroscopy

Correct Answer: C

The content explicitly states, 'Calorimetry experiments measure this heat transfer.' This is the definition of the technique.

Which statement best explains why adding 100 J of heat to 10 g of iron and 10 g of water will result in different final temperatures, assuming they start at the same initial temperature?

A) The first law of thermodynamics is not applicable to solids and liquids simultaneously.

B) Iron and water have differing specific heat capacities.

C) The process for water is endothermic, while the process for iron is exothermic.

D) Heating a system does not always increase its energy.

Correct Answer: B

The content states, 'The transfer of a given amount of thermal energy will not produce the same temperature change in equal masses of matter with differing specific heat capacities.' Since the masses and the heat added are equal, the only reason for a different temperature change is a difference in their specific heat capacities.

A positive value for 'q' in the context of a calorimetry calculation for a substance being heated or cooled signifies that:

A) The substance released heat to the surroundings.

B) The substance underwent a phase transition.

C) The substance absorbed heat from the surroundings.

D) The final temperature is lower than the initial temperature.

Correct Answer: C

The content states that one can 'calculate the heat q absorbed or released'. By convention, a positive q value indicates heat is absorbed by the system (an endothermic process), which corresponds to heating and an increase in the system's energy.

In a perfectly insulated calorimeter, a chemical reaction occurs that causes the temperature of the surrounding solution to increase. According to the first law of thermodynamics, which of the following must be true?

A) The energy gained by the solution is greater than the energy lost by the reaction.

B) The energy gained by the solution is equal to the energy released by the reaction.

C) The reaction is endothermic, absorbing energy from the solution.

D) The total energy of the calorimeter system (reaction + solution) has increased.

Correct Answer: B

The first law states that energy is conserved. In a perfectly insulated system, no energy can escape to the outside. Therefore, any energy that causes the solution's temperature to rise must have been released by the chemical reaction. The energy gained by the surroundings (solution) must equal the energy lost by the system (reaction).

The transfer of energy from a warmer body to a cooler body is identified in the text as an important form of:

A) Energy creation

B) Phase transition

C) Chemical reaction

D) Energy transfer

Correct Answer: D

The content directly states, 'The heating of a cool body by a warmer body is an important form of energy transfer.' This is the fundamental concept of heat flow.