"For water $\Delta$vap H = 41 kJ mol$-$1 at 373 K and 1 bar pressure. Assuming that water vapour is an ideal gas that occupies a much larger volume than liquid water, the internal energy change during evaporation of water is ___________ kJ mol$-$1[Use : R = 8.3 J mol$-$1 K$-$1]"

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Accepted Answer

"H₂O(l) $\to$ H₂O(g) : $\Delta$H = 41 ${{kJ} \over {mol}}$

$\Rightarrow$ From the relation : $\Delta$H = $\Delta$U + $\Delta$n_gRT

$\Rightarrow$ 41${{kJ} \over {mol}}$ = $\Delta$U + (1) $\times$ ${{8.3} \over {1000}}$ $\times$ 373

$\Delta$ DU = 41 $-$ 3.0959 = 38 kJ/mol"

For water $\Delta$_vap H = 41 kJ mol^$-$1 at 373 K and 1 bar pressure. Assuming that water vapour is an ideal gas that occupies a much larger volume than liquid water, the internal energy change during evaporation of water is ___________ kJ mol^$-$1

[Use : R = 8.3 J mol^$-$1 K^$-$1]

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For water $\Delta$vap H = 41 kJ mol$-$1 at 373 K and 1 bar pressure. Assuming that water vapour is an ideal gas that occupies a much larger volume than liquid water, the internal energy change during evaporation of water is ___________ kJ mol$-$1[Use : R = 8.3 J mol$-$1 K$-$1]

Solution

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For water $\Delta$_vap H = 41 kJ mol^$-$1 at 373 K and 1 bar pressure. Assuming that water vapour is an ideal gas that occupies a much larger volume than liquid water, the internal energy change during evaporation of water is ___________ kJ mol^$-$1

[Use : R = 8.3 J mol^$-$1 K^$-$1]