(A) . Work done in reversible isothermal expansion: $W = -nRT \ln(\frac{V_2}{V_1}) = -2 \times 8.314 \times 300 \times \ln(10) \approx -11488 \ J = -1

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(A) . Work done in reversible isothermal expansion: $W = -nRT \ln(\frac{V_2}{V_1}) = -2 \times 8.314 \times 300 \times \ln(10) \approx -11488 \ J = -11.5 \ kJ$. Magnitude is $11.5 \ kJ$ $(II)$.$B$. Work done in irreversible isothermal expansion: $W = -P_{ext}(V_2 - V_1) = -3 \times 10^3 \ Pa \times (3 - 1) \ m^3 = -6000 \ J = -6 \ kJ$. Magnitude is $6 \ kJ$ $(III)$.$C$. Change in internal energy: $\Delta U = nC_V \Delta T = 1 \times \frac{3}{2} \times 8.314 \times 320 \approx 3990 \ J \approx 4 \ kJ$. Magnitude is $4 \ kJ$ $(I)$.$D$. Change in enthalpy: $\Delta H = nC_P \Delta T = 1 \times \frac{5}{2} \times 8.314 \times 337 \approx 7004 \ J \approx 7 \ kJ$. Magnitude is $7 \ kJ$ $(IV)$.Thus,the correct match is $A-II, B-III, C-I, D-IV$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Difficult

Match the List-$I$ with List-$II$

List-$I$ Thermodynamic Process List-$II$ Magnitude in $kJ$

$A$. Work done in reversible,isothermal expansion of $2 \ mol$ of ideal gas from $2 \ dm^3$ to $20 \ dm^3$ at $300 \ K$. $I$. $4$

$B$. Work done in irreversible isothermal expansion of $1 \ mol$ ideal gas from $1 \ m^3$ to $3 \ m^3$ at $300 \ K$ against a constant pressure of $3 \ kPa$. $II$. $11.5$

$C$. Change in internal energy for adiabatic expansion of a $1 \ mol$ ideal gas with change of temperature $= 320 \ K$ and $\overline{C}_V = \frac{3}{2} R$. $III$. $6$

$D$. Change in enthalpy at constant pressure of $1 \ mole$ ideal gas with change of temperature $= 337 \ K$ and $\overline{C}_P = \frac{5}{2} R$. $IV$. $7$

Choose the correct answer from the option given below:

JEE MAIN 2026 All JEE MAIN

A
$A-II, B-III, C-I, D-IV$
B
$A-II, B-III, C-IV, D-I$
C
$A-I, B-II, C-III, D-IV$
D
$A-III, B-II, C-I, D-IV$

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List-$I$ Thermodynamic Process	List-$II$ Magnitude in $kJ$
$A$. Work done in reversible,isothermal expansion of $2 \ mol$ of ideal gas from $2 \ dm^3$ to $20 \ dm^3$ at $300 \ K$.	$I$. $4$
$B$. Work done in irreversible isothermal expansion of $1 \ mol$ ideal gas from $1 \ m^3$ to $3 \ m^3$ at $300 \ K$ against a constant pressure of $3 \ kPa$.	$II$. $11.5$
$C$. Change in internal energy for adiabatic expansion of a $1 \ mol$ ideal gas with change of temperature $= 320 \ K$ and $\overline{C}_V = \frac{3}{2} R$.	$III$. $6$
$D$. Change in enthalpy at constant pressure of $1 \ mole$ ideal gas with change of temperature $= 337 \ K$ and $\overline{C}_P = \frac{5}{2} R$.	$IV$. $7$

Similar Questions

Assertion : $\Delta H$ and $\Delta E$ are almost same for the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$.Reason : All reactants and products are gases.

The standard molar enthalpies of formation for ethane,$CO_2$,and water $(l)$ are $-21.1$,$-94.1$,and $-68.3 \text{ kcal/mol}$ respectively. What is the standard molar enthalpy of combustion for ethane in $\text{kcal/mol}$?

One mole of an ideal monoatomic gas at temperature $T$ expands adiabatically in an insulated flask from $1 \ L$ to $2 \ L$ against an external pressure of $1 \ atm$. What is the final temperature?

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Assertion : $\Delta H$ and $\Delta E$ are almost same for the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$.
Reason : All reactants and products are gases.