3. Enthalpy change is defined as a. the energy that is transferred into or out of a system when the pressure is constant and only P–Vwork is done. b. the change in internal energy of a system when the pressure is constant. c. the change in internal energy of a system when the volume is constant. d. the energy that is transferred into or out of a system when the pressure is constant and no work is done. e. the change in internal energy of a system when the pressure is constant and no work is done.

One mole of an ideal gas is contained in a cylinder with a movable piston. The temperature is constant at 77°C. Weights are removed suddenly from the piston to give the following sequence of three pressures. a. P, = 4.60 atm (initial state) b. P₂ = 2.73 atm c. P3 1.00 atm (final state) What is the total work (in joules) in going from the initial to the final state by way of the preceding two steps? J What would be the total work if the process were carried out reversibly?

Calculate the calorimeter constant for her calorimeter by following the steps below. 1. Calculate the mass of the warm water. 2. Calculate the change in temperature of the warm water. 3. Calculate the heat lost by the warm water. 4. Calculate the mass of the cold ocean water. 5. Calculate the change in temperature of the cold water. 6. Calculate the heat gained by the cold water. 7. Calculate the heat lost to the surroundings. 8. Calculate the calorimeter constant.

13. The enthalpy change, AH, of a process is defined as: The quantity of heat transferred in or out of a system as it undergoes a change at constant pressure. O The increase or decrease in temperature in a system. O The change in molecular disorder in a system. O The maximum amount of useful work that can be done in a system. 14. See image baln

1. State the first and second laws of thermodynamics

Which of the following best defines molar heat capacity. a. The quantity of heat required to raise the temperature of 1 mole of a substance by 1K   b. The quantity of heat required to lower the temperature of 1 liter of a substance by 1°C   c. The quantity of heat required to raise the temperature of 1 gram of a substance by 1°C   d. The quantity of heat required to raise the temperature of 1 gram of a substance by 1°F