Calculate change in enthalpy when 2 moles of liquid water at 1 bar and `100^(@)` C is coverted into steam at 2 bar and `300^(@)`. Assume `H_(2)O` vapoures to behave ideally.
[Latent heat of vaporisation of `H_(2)O(l)` at 1 bar and `100^(@)` C id=s 10.8 kcal per mole]
[R=`2cal//"mol" K`]

What is Delta U when 2.0 mole of liquid water vaporises at 100^(@)C ? The heat of vaporisation (Delta H_("vap".)) of water at 100^(@)C is 40.66 KJmol^(-1) .

What is Delta U when 2.0 mole of liquid water vaporises at 100^(@)C ? The heat of vaporisation (Delta H_("vap".)) of water at 100^(@)C is 40.66 KJmol^(-1) .

Calculate the work done when 1 mol of water vaporises at 100^(@)C and 1 atm pressure. Assume water vapour behaves like an ideal gas.

If water vapour is assumed to be a perfect gas, molar enthalpy change for vapouration of 1 mole of water at 1 bar and 100^(@)C is 41 kJ mol^(-1) . Calculate the internal energy change when a) 1 mol of water is vapourised at 1 bar and 100^(@)C b) 1 mol of water liquid is converted into ice.

If water vapour is assumed to be a perfect gas, molar enthalpy change for vaporization of 1 mol of water at 1 bar and 100^(@)C is 51 kJ mol ^(-1) . Calculate the internal energy, when 1 mol of water is vapourised at one bar pressure and 100^(@)C .

If water vapour is assumed to be a perfect gas, molar enthalpy change for vaporization of 1 mol of water at 1 bar and 100^(@) C is 41 kJ mol^(-1) . Calculate the internal energy, when 1 mol of water is vapourised at one bar pressure and 100^(@) C.

If water vapour is assumed to be a perfect gas, molar enthalpy change for vaporization of 1 mol of water at 1 bar and 100^(@) C is 41 kJ mol^(-1) . Calculate the internal energy, when 1 mol of water is vapourised at one bar pressure and 100^(@) C.