Consider the following processes: The temperatures of two identical gases are increased from the same initial temperature to the same final temperature.Reversible processes are used.For gas A the process is carried out at constant volume while for gas B it is carried out at constant pressure.The change in entropy:
A)is the same for A and B
B)is greater for A
C)is greater for B
D)is greater for A only if the initial temperature is low
E)is greater for A only if the initial temperature is high

Question

Quizplus · Accepted Answer

When a gas is heated at constant pressure, it expands and does work on the surroundings. The increase in volume leads to an increase in entropy. Therefore, the change in entropy is greater for gas B, which undergoes a constant pressure process. The change in entropy for constant volume processes (such as gas A) is given by: ΔS = q_rev / T, where q_rev is the heat absorbed during the reversible process. Since both gases are identical and undergo reversible processes, the heat absorbed and temperature change are the same for both gases, resulting in the same change in entropy for gas A and B. Thus, the answer is C, as the change in entropy is greater for gas B.

Consider the Following Processes: the Temperatures of Two Identical Gases