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ΔHvap for water is 40.7 KJ `mol^(−1)` . The entropy of vaporization of water is:
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delta h vap Standard enthalpy of vapourisation \Delta _ { \mathrm { vap } } \mathrm {
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delta h vap Standard enthalpy of vapourisation \Delta _ { \mathrm { vap } } \mathrm {
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If \Delta {H}{vap }^{\circ} for {H}{2} {O} is 44 {kJ} {mol}^{ 1}, then amount of heat required to evaporate 9 {~g} of {H}_{2} {O} is : 3. Using the approximate form of the Clausius Clapeyron Standard enthalpy of vapourisation \Delta _ { \mathrm { vap } } \mathrm {.. 5) For vaporization of water at 1 bar, \Delta H = 40.63 \mathrm {kJ} \ma..
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delta h vap Standard enthalpy of vapourisation \Delta _ { \mathrm { vap } } \mathrm {
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![For the vaporisation of water : `H_(2)O (I) hArr H_(2)O(g)` [1 atm. Pressure] Given : `Delta S = 120 JK^(-1)` and `Delta H =+45.0 kJ`. Evaluate the temperature at which liquid water](https://static.doubtnut.com/ss/web/12549322.webp "For the vaporisation of water : `H_(2)O (I) hArr H_(2)O(g)` [1 atm. Pressure] Given : `Delta S = 120 JK^(-1)` and `Delta H =+45.0 kJ`. Evaluate the temperature at which liquid water")
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