One mole of a perfect gas expands isothermally and reversibly from $10 \mathrm{~dm}^3$ to $20 \mathrm{~dm}^3$ at $300 \mathrm{~K}$. $\Delta u, q$ and work done in the process are $\left[\mathrm{R}={8 . 3} \times {1 0}^{-{3}}\,\mathrm\,\,{kJ} \mathrm{K}^{-1} \mathrm{~mol}^{-{1}}\right]$

$0,17.48 \mathrm{~J}, 1.726 \mathrm{~J}$

$0,21.84 \mathrm{~kJ}, 21.84 \mathrm{~kJ}$

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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One mole of a perfect gas expands isothermally and reversibly from

10 \mathrm{~dm}^3

20 \mathrm{~dm}^3

300 \mathrm{~K}

\Delta u, q

and work done in the process are

\left[\mathrm{R}={8 . 3} \times {1 0}^{-{3}}\,\mathrm\,\,{kJ} \mathrm{K}^{-1} \mathrm{~mol}^{-{1}}\right]

View answer and explanation

Correct option: A

0,1.726 \mathrm{~kJ},-1.726 \mathrm{~kJ}

Option A (0, 1.726 kJ, -1.726 kJ) is correct because in an isothermal process, the change in internal energy is zero, and the heat absorbed is equal to the negative of the work done.

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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