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Determine the value of DeltaH and DeltaU...

Determine the value of `DeltaH` and `DeltaU` for the reversible isothermal evaporation of 90.0g of water at `100^(@)C`.Assume that water vapour behaves as an ideal gas and heat of evaporation of water is `540 calg^(-)R = 2.0 cal mol^(-1)K^(-1)`.

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44.87 kcal, 48.6 kcal
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Determine the value of DeltaH and DeltaU for the reversible isothermal evaporation of 90.0g of water at 100^(@)C . Assume that water behaves as an ideal gas and heat of evaporation of water is 540 cal g^(-1) (R = 2.0 cal mol^(-1)K^(-1)) .

What is the value of DeltaE (heat change at constant volume)for reversible isothermal evaporation of 90g water at 100^(@)C Assuming water vapour behaves as an ideal gas and (DeltaH_("vap"))_("water")=540calg^(-1)

What is value of DeltaU for reversible isothernal evaporation of 90g water at 100^(@)C ? Assuming water vapour behaves as an ideal gas, Delta_(vap. Water)H = 540cal g^(-1)

What is the value of Delta H for a reversible isothermal evaporation of 180g of water at 100^(@)C ? Latent ehat of evaporation of water =539.7 cal K^(-1)g^(-1) ?

The value of (DeltaH- DeltaU) for vaporisation of water at 100^@C is 'x' x 10^2 J//"mole" , assume water vapour to be an ideal gas [Take R = 8.31 J//"mole".K ]

Find the amount of heat required to convert 10g of water at 100^(@)C into steam. (Spefic latent heat of vaporization of water = 540 cal //g )

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