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The latent heat of vapourisation of water is $2240 \mathrm{~J}$. If the work done in the process of vapourisation of $1 \mathrm{~g}$ is $168 \mathrm{~J}$, then increase in internal energy is
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$2072 \mathrm{~J}$
Latent heat of vapourisation of water $(L)=2240 \mathrm{~J}$, mass of the water $(\mathrm{m})=1 \mathrm{~g}$ and work done $(d W)=168 \mathrm{~J}$
From first law of thermodynamics, heat supplied in vapourisation $(d Q)=m L=d U+d W$ or or
$$
\begin{aligned}
& 1 \times 2240=d U+168 \\
& d U=2240-168=2072 \mathrm{~J}
\end{aligned}
$$
(where $d U=$ increase in internal energy).
From first law of thermodynamics, heat supplied in vapourisation $(d Q)=m L=d U+d W$ or or
$$
\begin{aligned}
& 1 \times 2240=d U+168 \\
& d U=2240-168=2072 \mathrm{~J}
\end{aligned}
$$
(where $d U=$ increase in internal energy).
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