In Figure 1, we have a box of gas that contains a paddle which, when turned, does work on the surroundings. The box initially has a partition, and one mole of gas is contained only on one side. When the partition is broken, the gas will move to occupy the entire box. The gas is heated such that it has a constant temperature. (hint: Assume the gas is an ideal gas. For such a gas, its internal energy is a function purely of its temperature and not its volume and pressure.) a) How much work will the gas do on the surroundings? b) How much heat did it add to the gas during this process? c) What is the gain in entropy of the system? d) The entropy increase is the loss of energy per unit temperature that is available to do work. The amount of energy that is no longer available to do work is Q = ST. After this process, how much heat will be available to 1 do work? Does your answer make physical sense? How much work could be done, thinking about this conceptually, after this process?

In Figure 1, we have a box of gas that contains a paddle which, when turned, does work on the surroundings. The box initially has a partition, and one mole of gas is contained only on one side. When the partition is broken, the gas will move to occupy the entire box. The gas is heated such that it has a constant temperature. (hint: Assume the gas is an ideal gas. For such a gas, its internal energy is a function purely of its temperature and not its volume and pressure.) a) How much work will the gas do on the surroundings? b) How much heat did it add to the gas during this process? c) What is the gain in entropy of the system? d) The entropy increase is the loss of energy per unit temperature that is available to do work. The amount of energy that is no longer available to do work is Q = ST. After this process, how much heat will be available to 1 do work? Does your answer make physical sense? How much work could be done, thinking about this conceptually, after this process?