Given below are two statements:
Statement 1 : For an ideal gas, heat capacity at constant volume is always greater than the heat capacity at constant pressure.
Statement II : In a constant volume process, no work is produced and all the heat withdrawn goes into the chaotic motion and is reflected by a temperature increase of the ideal gas.
In the light of the above statements, choose the correct answer from the options given below
Select the correct option:
A
Both Statement I and Statement II are true
B
Both Statement I and Statement II are false
C
Statement I is true but Statement II is false
D
Statement I is false but Statement II is true
✓ Correct! Well done.
✗ Incorrect. Try again or view the solution.
Solution
From first law of thermodynamics
$$
\Delta \mathrm{U}=\mathrm{q}+\mathrm{w}
$$
constant volume $\mathrm{w}=0$
$$
\Delta \mathrm{U}=\mathrm{q}
$$
Also $\mathrm{C}_{\mathrm{P}}=\mathrm{C}_{\mathrm{V}}+\mathrm{R}$, So, $\mathrm{C}_{\mathrm{P}}>\mathrm{C}_{\mathrm{V}}$
Here, $\mathrm{C}_{\mathrm{P}}=$ heat capacity at constant pressure
$\mathrm{C}_{\mathrm{v}}=$ Heat capacity at constant volume.
R = constant
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