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Jobin Rao Memon
Asked: 2022-11-03T21:51:33+05:30 In:

If water vapour is assumed to be a perfect gas, molar enthalpy change for vaporization of 1 mol of water at 1 bar and `100^(@)`C is 41 kJ `mol^(-1)`. Calculate the internal energy, when 1 mol of water is vapourised at one bar pressure and `100^(@)`C.

If water vapour is assumed to be a perfect gas, molar enthalpy change for vaporization of 1 mol of water at 1 bar and `100^(@)`C is 41 kJ `mol^(-1)`. Calculate the internal energy, when 1 mol of water is vapourised at one bar pressure and `100^(@)`C.
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  1. The change `H_(2)O(I) rarr H_(2)O(g)`
    `Delta H = Delta U + n_(g)RT`
    `or Delta U = Delta H – Delta n_(g)RT`
    = 41 kJ `mol^(-1) – 1 xx “8.314 J”” ” mol^(-1)K^(-1)xx 373 K`
    = 41 kJ `mol^(-1)` – 3101 J `mol^(-1)`
    = 41 kJ`mol^(-1)` – 3.101 kj `mol^(1)`
    = 37.9 kJ `mol^(-1)`

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