Question 1

Which of the following is a state function in thermodynamics?

Accepted Answer

Internal energy ($$U)$$

Question 2

A chemical reaction is performed in a bomb calorimeter. Which of the following statements is TRUE about the conditions inside the calorimeter?

Accepted Answer

The reaction occurs at constant volume.

Question 3

Which equation correctly relates the change in internal energy ($$\Delta U) to $$heat ($$q) $$and work ($$w$$)?

Accepted Answer

$$\Delta U = q + w$$

Question 4

A student burns 1.00 g of glucose ($$C_6H_{12}O_6$) in a bomb calorimeter. The temperature of the calorimeter increases by 2.50$$^\circ C$$. If the heat capacity of the calorimeter is 4.00$$ 	ext{ kJ}/^\circ C$$, what is the heat released (q$) by the reaction?

Accepted Answer

$$q = 10.0 	ext{ kJ}$$

Question 5

Which of the following best describes an exothermic process?

Accepted Answer

Heat flows out of the system to the surroundings.

Question 6

Which formula is used to calculate the heat absorbed or released by a substance when its temperature changes?

Accepted Answer

$$q = mC_p \Delta T$$

Question 7

If a reaction is performed at constant pressure, which thermodynamic quantity is measured by a coffee cup calorimeter?

Accepted Answer

Change in enthalpy ($$\Delta H)$$

Question 8

A system does $$50 	ext{ J} of $$work on the surroundings and absorbs $$120 	ext{ J} of $$heat. What is the change in internal energy ($$\Delta U) of $$the system?

Accepted Answer

$$\Delta U = 70 	ext{ J}$$

Question 9

Which of the following is NOT a limitation of calorimetry?

Accepted Answer

Accurate measurement of temperature change

Question 10

Which statement about state functions is correct?

Accepted Answer

State functions depend only on the initial and final states.

Question 11

Which of the following processes is endothermic?

Accepted Answer

Melting of ice

Question 12

In a bomb calorimeter, which equation correctly relates the change in internal energy to the heat released?

Accepted Answer

$$\Delta U = q_v$$

Question 13

Which of the following is TRUE about the first law of thermodynamics?

Accepted Answer

The total energy of an isolated system is constant.

Question 14

A reaction occurs at constant pressure and produces a gas. Which equation should be used to calculate the enthalpy change ($$\Delta H$$)?

Accepted Answer

$$\Delta H = \Delta U + P \Delta V$$

Question 15

Which of the following is the correct expression for work done by a gas during expansion at constant pressure?

Accepted Answer

$$w = -P \Delta V$$

Question 16

A sample of NaCl is dissolved in water in a coffee cup calorimeter. The temperature of the solution decreases. What can you conclude about the process?

Accepted Answer

The dissolution of NaCl is endothermic.

Question 17

Which of the following is TRUE about specific heat capacity ($$C$$)?

Accepted Answer

It is the amount of heat required to raise the temperature of 1 gram of a substance by $$1^\circ C.$$

Question 18

Which of the following reactions represents the standard enthalpy of formation ($$\Delta H_f^\circ) $$for sodium chloride?

Accepted Answer

$$Na (s) + \frac{1}{2}Cl_2$ (g) \rightarrow NaCl (s)$$

Question 19

Which of the following statements about enthalpy ($$\Delta H) is $$correct?

Accepted Answer

Enthalpy change at constant pressure equals the heat exchanged.

Question 20

A reaction in a coffee cup calorimeter causes the temperature of the solution to increase by $$3.0^\circ C. $$The solution has a mass of $$100 	ext{ g}$$ and a specific heat capacity of $$4.18 	ext{ J}/	ext{g}^\circ C. $$What is the heat absorbed by the solution?

Accepted Answer

$$q = 1254 	ext{ J}$$

Thermodynamics and Calorimetry in General Chemistry

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