Consider the following volume-temperature $( V - T )$ diagram for the expansion of $5$ moles of an ideal monoatomic gas.
Considering only $P-V$ work is involved, the total change in enthalpy (in Joule) for the transformation of state in the sequence $X \rightarrow Y \rightarrow Z$ is $\qquad$
[Use the given data: Molar heat capacity of the gas for the given temperature range, $C _{ v , m }=12 J K ^{-1} mol ^{-1}$ and gas constant, $R =8.3 J K ^{-1} mol ^{-1}$ ]
IIT 2024, Advanced
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For ideal gas
$\Delta H=n C_P \Delta T$
$\because \quad C_P=C_V+R=12+8.3=20.3 J / K \text {-mole }$
$\therefore \Delta H=5 \times 20.3 \times(415-335)$
$\Delta H=8120 \text { Joule }$
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