2 mole of an ideal gas at $27^{\circ} C$ expands iso - thermally and reversibly from a volume of 4 litre to 40 litre. The work done(in kJ)by the gas is:

$w = - 28.72 k J$

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$w = - 11.488 k J$

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$w = - 5.736 k J$

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$w = - 4.988 k J$

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Solution

The correct option is B
$w = - 11.488 k J$

$n = 2, T = 300 K, V_{2} = 40 l i t, V_{1} = 4 l i t, R = 8.314 / K / m o l$

Amount of work done is reversible isothermal expension

$W = - 2.303 n R T l o g (\frac{V_{2}}{V_{1}}) = - 2.303 \times 2 \times 8.314 \times 300 \times l o g (\frac{40}{4}) = - 11.488 k J$

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2 mole of an ideal gas at 27∘C expands iso - thermally and reversibly from a volume of 4 litre to 40 litre. The work done(in kJ)by the gas is:

The correct option is B w = −11.488 kJ n = 2,T = 300 K,V2 = 40 lit,V1 = 4 lit,R = 8.314/K/mol Amount of work done is reversible isothermal expension W = −2.303nRTlog(V2V1) = −2.303 × 2 × 8.314 × 300 × log(404) = −11.488kJ

2 mole of an ideal gas at $27^{\circ} C$ expands iso - thermally and reversibly from a volume of 4 litre to 40 litre. The work done(in kJ)by the gas is: