Given that $1\,g$ of water in liquid phase has volume $1\,cm^3$ and in vapour phase $1671\, cm^3$ at atmospheric pressure and the latent heat of vaporization of water is $2256\,J/g;$ the change in the internal energy in joules for $1\,g$ of water at $373\,K$ when it changes from liquid phase to vapour phase at the same temperature is ....... $J$
JEE MAIN 2013,NEET 2019, Medium
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$W = P\left( {dV} \right)$$ = 0.01 \times {10^5}\left( {1671 - 1} \right) \times {10^{ - 6}} = 167\,J$
$Q = \Delta U + W$
$\Delta U = Q - W = mL - 167$$ = 2256 - 167 = 2089\,J$
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