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90 g of water spilled out from a vessel ...

90 g of water spilled out from a vessel in the room on the floor. Assuming that water vapour behaving as an ideal gas, calculate the internal energy change when the spilled water undergoes complete evaporation at `100^(@)C`. (Given the molar enthalpy of vaporisation of water at 1 bar and 373 K = 41 kJ `mol^(-1)`).

Text Solution

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`5H_(2)O(I) rightarrow 5H_(2)O(v)`
`Delta E = Delta H - Delta n RT`
` = 41 xx5 xx-5 xx8314 xx10^(-3) xx373 `
`Delta E = 189.5 kJ`
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