The heat capacity of a substance can be measured under either constant volume or constant pressure conditions. Which of the following sets of relationships between (heat capacity under constant volume conditions) and (heat capacity under constant pressure conditions) are always true?
Suppose 2 moles of water at 333 K are added to 4 moles of water at 293 K. What would the entropy change associated with this process be, assuming that there is no exchange of heat with the surroundings? (The heat capacity of water is and may be considered to be independent of temperature.)
Two 1 mol blocks of aluminum, one at 273 K and the other at 373 K, are brought into thermal contact. What will the temperature of the two blocks be when they have reached thermal equilibrium? What will the total entropy change that accompanies the thermal equilibration process be? Assume that the two blocks of aluminum are in a container with walls that keep them completely isolated from outside surroundings, and take the heat capacity of the aluminum blocks to be .