A small amount of heat Q flows out of a hot system A (at T_hot = 360 K) into a c
ID: 1638252 • Letter: A
Question
A small amount of heat Q flows out of a hot system A (at T_hot = 360 K) into a cold system B (at T_cold = 230 K). The overall [AB] system is the thermally isolated from the rest of the universe. (Q is small enough that the temperature changes of the objects can be ignored.) The figure shows an example of this process (but with 7_hot = 350 K and T_cold = 250 K -- do not use the temperatures in the figure). Do you exp the entropy change of the [AB] system to be positive, negative, or zero? Explain why you think so. Since the system Isolated, entropy always increases. Also if we try to solve mathematically delta delta = QT. Ta = (Q/T) because the heat loft box A If Q = [5], mA = 1.2 kg, and m_B = 0.6 kg, find the total change in the entropy of the [AB] system, Delta S_AB. Suppose we let the two objects come to a thermal equilibrium, Do you expect the total Gibbs free energy of the [AB] system to have increased, decreased, or remained the same? Explain why you think so. This answer has not been graded yet.Explanation / Answer
2) Change in entropy of AB = change in entropy of A + change in entropy of B
= -0.5/360 + 0.5/230
= 0.000785 J/K answer
Here the entropy change in B is more positive