Match the LIST-I with LIST-II, Thermodynamic Process [2026]

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Solution

Q.
Match the LIST-I with LIST-II [2026]

List-I List-II

Thermodynamic Process 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 ${\bar{C}}_{V} = \frac{3}{2} R$ . III. 6

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

Choose the correct answer from the options given below:

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

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

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

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

Ans.
(1)

$Option (A)$

$W = - n R T \ln \frac{V_{2}}{V_{1}}$

$= \frac{- 2 \times 8.314 \times 300}{1000} \times \ln (\frac{20}{2}) kJ$

$= - 11.5 kJ$

$Option (B)$

$W = - P_{ext} [V_{2} - V_{1}]$

$= - 3 [3 - 1]$

$= - 6 kJ$

$Option (C)$

$Δ U = n C_{v} Δ T$

$= 1 \times \frac{3}{2} \times \frac{8.314 \times 320}{1000} kJ$

$= 3.99 kJ$

$Option (D)$

$Δ H = n C_{p} Δ T$

$= 1 \times \frac{5}{2} \times \frac{8.314 \times 337}{1000} kJ$

$= 7 kJ$

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