(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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$A$ sample of gas is compressed from an initial volume of $2V_0$ to $V_0$ using three different processes.
First: Using reversible isothermal.
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Third: Using irreversible adiabatic under a constant external pressure.
Then

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Consider the reversible processes for $1.0 \ mol$ of an ideal gas. $w_1, w_2, w_3$ and $w_4$ represent work done (in calories) in the processes $1, 2, 3$ and $4$, respectively; $\Delta U_2$ and $\Delta U_4$ are changes in the internal energy for the processes $2$ and $4$, respectively. (use $R = 2 \ cal \ K^{-1} \ mol^{-1}$). The correct option is:

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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.

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Five moles of a gas are subjected to a series of changes as shown in the given graph. What are the processes $A \rightarrow B$,$B \rightarrow C$,and $C \rightarrow A$ respectively?

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Given below are two statements:
Statement $I$: For an ideal gas, heat capacity at constant volume is always greater than the heat capacity at constant pressure.
Statement $II$: In a constant volume process, no work is produced and all the heat withdrawn goes into the chaotic motion and is reflected by a temperature increase of the ideal gas.

MediumJEE MAIN 2026

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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 $\overline{C}_P = \frac{5}{2} R$.	$IV$. $7$

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$A$ sample of gas is compressed from an initial volume of $2V_0$ to $V_0$ using three different processes.First: Using reversible isothermal.Second: Using reversible adiabatic.Third: Using irreversible adiabatic under a constant external pressure.Then

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