A sample of $0.1\, g$ of water at $100^o C$ and normal pressure $(1.013 \times 10^5 N m^{-2} )$ requires $54\ cal $ of heat energy to convert to steam at $100^o C.$ If the volume of the steam produced is $167.1 \,cc,$ the change in internal energy of the sample, is ....... $J$
NEET 2018, Medium
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Using first law of thermodynamics,
$\Delta Q = \Delta U + \Delta W$
$ \Rightarrow 54 \times 4.18 = \Delta U + 1.013 \times {10^5}\left( {167.1 \times {{10}^{ - 6}} - 0} \right)$
$ \Rightarrow \Delta U = 208.7\,J$
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