What is the work done in cal during the rever | vedclass

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(D) For an ideal gas,the number of moles $(n) = 1$; initial pressure $(P_1) = 10 \, atm$; final pressure $(P_2) = 1 \, atm$. Constant absolute tempera

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$-1381.8$

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(D) For an ideal gas,the number of moles $(n) = 1$; initial pressure $(P_1) = 10 \, atm$; final pressure $(P_2) = 1 \, atm$. Constant absolute temperature $(T) = 300 \, K$; gas constant $(R) = 2 \, cal \, mol^{-1} \, K^{-1}$. The work done $(W)$ for the reversible isothermal expansion of an ideal gas is given by: $W = -2.303 \, nRT \, \log_{10} \left( \frac{P_1}{P_2} ight)$ $W = -2.303 	imes 1 	imes 2 	imes 300 	imes \log_{10} \left( \frac{10}{1} ight)$ $W = -2.303 	imes 600 	imes 1$ $W = -1381.8 \, cal$

What is the work done in $cal$ during the reversible isothermal expansion of $1 \, mol$ of an ideal gas at $300 \, K$ from $10 \, atm$ to $1 \, atm$?

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