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Question

Calculate the work done (in Joules) when 0.2 mole of an ideal gas at 300K expands isothermally and reversibly from an initial volume of 2.5 liters to the final volume of 25 liters.

A
996
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B
1148
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C
11.48
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D
897
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Solution

The correct option is B −1148Solution:- (B) −1148As we know that, work done in an isothermal reversible expansion is given as-W=−2.303×nRT×logVfViGiven:-n=0.2 molT=300KR=8.314J/K−molVf=25LVi=2.5LW=−2.303×0.2×8.314×300×log252.5⇒W=−1148.83J≈−1148JHence the work done is −1148J.

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