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

Question

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 $X \to Y \to Z$ is ________. [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, $R = 8.3 J K^{- 1} mol^{- 1}]$

TestHub · Accepted Answer

For ideal gas Δ H = nC P ​ Δ T ∵ C P ​ = C V ​ + R = 12 + 8.3 = 20.3 J / K -mole ∴ Δ H = 5 × 20.3 × ( 415 − 335 ) Δ H = 8120 Joule

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