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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/791383.webp)
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delta h vap Solved: For the reversible vaporization of water at $$100^0C$$ and 1 atmospheric pressure, $$Delta [Physics]
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delta h vap Solved: For the reversible vaporization of water at $$100^0C$$ and 1 atmospheric pressure, $$Delta [Physics]
![delta h vap Solved: For the reversible vaporization of water at $$100^0C$$ and 1 atmospheric pressure, $$Delta [Physics] main image 0](https://www.researchgate.net/publication/329858807/figure/tbl1/AS:706503958880258@1545455078670/Calculated-and-Experimental-Enthalpies-D-vap-H-and-D-vap-H-exp-of-Vaporization-in-kJ-mol.png)
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Hvap for water is 40.7 KJ `mol^(1)` . The entropy of vaporization of water is: Calculation of Enthalpy of Vaporization at a Given Temperature Video answer for \Delta_{\text {vap }} \mathrm{H}^{\Theta} for water is +40.79 \mathrm{kJ} \mathrm{mol}^{ 1} at 1 bar and 100^{\circ} \mathrm{C}. Change in internal energy for this vapourisation under vp vs temp.svg The difference between `Delta`H and `Delta`U at constant volume is equal to
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delta h vap Solved: For the reversible vaporization of water at $$100^0C$$ and 1 atmospheric pressure, $$Delta [Physics]
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