(C) For an isothermal reversible expansion of an ideal gas,the work done is given by the formula $w = - nRT \ln \frac{V_2}{V_1}$.Option $A$ is correct

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$w = nRT \ln \frac{V_2}{V_1}$ (isothermal reversible expansion of an ideal gas)

(C) For an isothermal reversible expansion of an ideal gas,the work done is given by the formula $w = - nRT \ln \frac{V_2}{V_1}$.Option $A$ is correct because for an ideal gas,internal energy $U$ is a function of temperature only,so $\Delta U = 0$ for isothermal processes.Option $B$ is the correct formula for work done.Option $C$ is incorrect because it lacks the negative sign,which represents work done by the system.Option $D$ is correct because at constant volume,$w = 0$,so $\Delta U = q_v$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

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Which of the following statements or relationships is not correct in thermodynamic changes?

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A
$\Delta U = 0$ (isothermal reversible expansion of a gas)
B
$w = - nRT \ln \frac{V_2}{V_1}$ (isothermal reversible expansion of an ideal gas)
C
$w = nRT \ln \frac{V_2}{V_1}$ (isothermal reversible expansion of an ideal gas)
D
For a system of constant volume,heat involved directly changes to internal energy.

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For the reaction $X_2O_{4(g)} \to 2XO_{2(g)}$,given $\Delta U = 2.1 \, kcal$ and $\Delta S = 20 \, cal \, K^{-1}$ at $300 \, K$. Calculate $\Delta G$ in $kcal$.

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For a hypothetical reaction $A_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{(g)}$,at $200 \ K$,$\Delta_r G$ and $\Delta_r S$ are $20 \ kJ \ mol^{-1}$ and $-20 \ J \ K^{-1} \ mol^{-1}$ respectively. If $\Delta_r C_p = 20 \ J \ K^{-1} \ mol^{-1}$,find $\Delta_r H$ at $400 \ K$ in $kJ \ mol^{-1}$.

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For the reaction $CO_{(g)} + \frac{1}{2}O_{2_{(g)}} \rightarrow CO_{2_{(g)}}$ at $17^o C$ and constant volume,the heat of reaction is $-67.71 \, K \, cal$. What is the heat of reaction at constant pressure at $17^o C$ in $K \, cal$?

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The process of evaporation of a liquid is completed by .......

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Given below are two statements:
Statement-$I$: For isothermal irreversible change of an ideal gas,$q = -w = P_{\text{ext}} (V_{\text{final}} - V_{\text{initial}})$
Statement-$II$: For adiabatic change,$\Delta U = W_{\text{adiabatic}}$
The correct answer is

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Which of the following statements or relationships is not correct in thermodynamic changes?

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For the reaction $X_2O_{4(g)} \to 2XO_{2(g)}$,given $\Delta U = 2.1 \, kcal$ and $\Delta S = 20 \, cal \, K^{-1}$ at $300 \, K$. Calculate $\Delta G$ in $kcal$.

For a hypothetical reaction $A_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{(g)}$,at $200 \ K$,$\Delta_r G$ and $\Delta_r S$ are $20 \ kJ \ mol^{-1}$ and $-20 \ J \ K^{-1} \ mol^{-1}$ respectively. If $\Delta_r C_p = 20 \ J \ K^{-1} \ mol^{-1}$,find $\Delta_r H$ at $400 \ K$ in $kJ \ mol^{-1}$.

For the reaction $CO_{(g)} + \frac{1}{2}O_{2_{(g)}} \rightarrow CO_{2_{(g)}}$ at $17^o C$ and constant volume,the heat of reaction is $-67.71 \, K \, cal$. What is the heat of reaction at constant pressure at $17^o C$ in $K \, cal$?

The process of evaporation of a liquid is completed by .......

Given below are two statements:Statement-$I$: For isothermal irreversible change of an ideal gas,$q = -w = P_{\text{ext}} (V_{\text{final}} - V_{\text{initial}})$Statement-$II$: For adiabatic change,$\Delta U = W_{\text{adiabatic}}$The correct answer is

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Given below are two statements:
Statement-$I$: For isothermal irreversible change of an ideal gas,$q = -w = P_{\text{ext}} (V_{\text{final}} - V_{\text{initial}})$
Statement-$II$: For adiabatic change,$\Delta U = W_{\text{adiabatic}}$
The correct answer is