(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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Assertion $(A)$: If heat of combustion of $C_2H_6$ is $X \ kJ \ mol^{-1}$,heat liberated on combustion of $150 \ g$ of $C_2H_6$ is $5X \ kJ$.
Reason $(R)$: Enthalpy is an extensive property.

MediumAP EAMCET 2017

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The energy of combustion per mole of $H_2$,$LPG$,and octane follows the order:

DifficultKVPY 2021

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Match the following:
List-$I$ List-$II$
$(A) \Delta U = W_{ad}$ $I.$ Isothermal reversible expansion
$(B) \Delta U = q - W$ $II.$ Wall is adiabatic
$(C) \Delta U = -q$ $III.$ Thermally conducting walls
$(D) \Delta U = 0$ $IV.$ Isolated system
$V.$ Closed system

The correct answer is

List-$I$	List-$II$
$(A) \Delta U = W_{ad}$	$I.$ Isothermal reversible expansion
$(B) \Delta U = q - W$	$II.$ Wall is adiabatic
$(C) \Delta U = -q$	$III.$ Thermally conducting walls
$(D) \Delta U = 0$	$IV.$ Isolated system
	$V.$ Closed system

EasyAP EAMCET 2019

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Two liters of $N_2$ gas at $0 \, ^\circ C$ and $5 \, atm$ pressure undergoes isothermal expansion against a constant external pressure of $1 \, atm$ until the pressure of the gas becomes $1 \, atm$. If the gas is ideal,what is the work done in the expansion in $J$?

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What is the enthalpy of vaporization of ethanol in $kJ/mol$? Given: boiling point $(b.p.)$ = $79.5 \, ^\circ C$ and entropy change $(\Delta S_{vap})$ = $109.8 \, J K^{-1} mol^{-1}$.

Medium

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

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Assertion $(A)$: If heat of combustion of $C_2H_6$ is $X \ kJ \ mol^{-1}$,heat liberated on combustion of $150 \ g$ of $C_2H_6$ is $5X \ kJ$.Reason $(R)$: Enthalpy is an extensive property.

The energy of combustion per mole of $H_2$,$LPG$,and octane follows the order:

Match the following:List-$I$List-$II$$(A) \Delta U = W_{ad}$$I.$ Isothermal reversible expansion$(B) \Delta U = q - W$$II.$ Wall is adiabatic$(C) \Delta U = -q$$III.$ Thermally conducting walls$(D) \Delta U = 0$$IV.$ Isolated system$V.$ Closed systemThe correct answer is

Two liters of $N_2$ gas at $0 \, ^\circ C$ and $5 \, atm$ pressure undergoes isothermal expansion against a constant external pressure of $1 \, atm$ until the pressure of the gas becomes $1 \, atm$. If the gas is ideal,what is the work done in the expansion in $J$?

What is the enthalpy of vaporization of ethanol in $kJ/mol$? Given: boiling point $(b.p.)$ = $79.5 \, ^\circ C$ and entropy change $(\Delta S_{vap})$ = $109.8 \, J K^{-1} mol^{-1}$.

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Assertion $(A)$: If heat of combustion of $C_2H_6$ is $X \ kJ \ mol^{-1}$,heat liberated on combustion of $150 \ g$ of $C_2H_6$ is $5X \ kJ$.
Reason $(R)$: Enthalpy is an extensive property.

Match the following:
List-$I$ List-$II$
$(A) \Delta U = W_{ad}$ $I.$ Isothermal reversible expansion
$(B) \Delta U = q - W$ $II.$ Wall is adiabatic
$(C) \Delta U = -q$ $III.$ Thermally conducting walls
$(D) \Delta U = 0$ $IV.$ Isolated system
$V.$ Closed system

The correct answer is