Question:

Two thermodynamical processes are shown in the figure. The molar heat capacity for process A A and B B are CA C_A and CB C_B . The molar heat capacity at constant pressure and constant volume are represented by CP C_P and CV C_V , respectively. Choose the correct statement.
Figure

Updated On: Jan 9, 2025
  • CB=,CA=0 C_B = \infty, \, C_A = 0
  • CA=0andCB= C_A = 0 \, \text{and} \, C_B = \infty
  • CP>CV>CA=CB C_P > C_V > C_A = C_B
  • CA>CP>CV C_A > C_P > C_V
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The Correct Option is B

Solution and Explanation

Step 1. Understanding the Slopes in the log P vs. log V Diagram:

Process A has a slope of tan1γ \tan^{-1} \gamma , where γ=CPCV \gamma = \frac{C_P}{C_V} , indicating an adiabatic process (since PVγ=constant PV^\gamma = \text{constant} ). Process B has a slope of 45 45^\circ or tan11 \tan^{-1} 1 , suggesting that it is an isothermal process (since PV=constant PV = \text{constant} ).

Step 2. Using Heat Capacities for Adiabatic and Isothermal Processes:

For an adiabatic process (PVγ=constant PV^\gamma = \text{constant} ), the heat capacity CA C_A is effectively zero because no heat exchange occurs (dQ=0 dQ = 0 for adiabatic). For an isothermal process (PV=constant PV = \text{constant} ), the heat capacity CB C_B tends to infinity because any heat added is used to perform work without changing temperature.

Conclusion:

Therefore, the correct statement is:

CA=0andCB= C_A = 0 \quad \text{and} \quad C_B = \infty

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