1 mole of an ideal gas is expanded isothermally at 298 K until its volume is tripled. Find the value of ${ΔS}_{total}$ in joule when expansion is carried out irreversibly when 836.8 J of heat is less absorbed then in corresponding reversible expansion.

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answer is 2.81.

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Detailed Solution

$Q_{ir} = Q_{rev} - 836.8 J \begin{array}{l} {ΔS}_{total} = {ΔS}_{sys} + {ΔS}_{sur} = \frac{Q_{r e v}}{298} + (- \frac{Q_{i r}}{298}) = \frac{836.8}{298} = 2.808 J = 2.81 J \end{array}$

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