If 5 moles of an ideal gas expands from $10 \mathrm{~L}$ to a volume of $100 \mathrm{~L}$ at $300 \mathrm{~K}$ under isothermal and reversible condition then work, $\mathrm{w}$, is $-x \mathrm{~J}$. The value of $x$ is __________.
(Given R = 8.314 J K$^{-1}$ mol$^{-1}$)
Answer (integer)
28721
Solution
<p>It is isothermal reversible expansion, so work done negative</p>
<p>$$\begin{aligned}
& \mathrm{W}=-2.303 \mathrm{nRT} \log \left(\frac{\mathrm{V}_2}{\mathrm{~V}_1}\right) \\
& =-2.303 \times 5 \times 8.314 \times 300 \log \left(\frac{100}{10}\right) \\
& =-28720.713 \mathrm{~J} \\
& \equiv-28721 \mathrm{~J}
\end{aligned}$$</p>
About this question
Subject: Chemistry · Chapter: Thermodynamics · Topic: Zeroth and First Law
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