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At $25^{\circ} \mathrm{C}$, when 1 mole of butane is heated, $\mathrm{CO}_2$ and liquid $\mathrm{H}_2 \mathrm{O}$ are formed, then the work done is
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$85.6 \mathrm{~L}$ atm
$\begin{aligned} & \text { } \mathrm{C}_4 \mathrm{H}_{10(g)}+\frac{13}{2} \mathrm{O}_{2(g)} \longrightarrow 4 \mathrm{CO}_{2(g)}+5 \mathrm{H}_2 \mathrm{O}_{(l)} \\ & \Delta n_g=4-\left(1+\frac{13}{2}\right)=-\frac{7}{2} \\ & w=-\Delta n_g R T=-\left(-\frac{7}{2} \times 0.0821 \times 298\right) \\ & =85.63 \mathrm{~L} \mathrm{~atm}\end{aligned}$
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