Calculate the temperature at which liquid water will be in equilibrium with water vapour.
`DeltaH_(vap)=40.73kJ" "mol^(-1) and DeltaS_(vap)=0.109kJ" "mol^(-1)" "K^(-1)`

Calculate the temperature at which liquid water will be in equilibrium with water vapour. Delta_(vap)H = 40.00 kJ mol^(-1) and Delta_(vap)S = 0.100 kJ mol^(-1)K^(-1)

At what temperature liquid water will be in equilibrium with water vapour? DeltaH_("vap")="40.73 kJ mol"^(-1),DeltaS_("vap")="0.109 kJ K"^(-1)"mol"^(-1)

At what temperature liquid water will be in equilibrium with water vapour? DeltaH_("vap")="40.73 kJ mol"^(-1),DeltaS_("vap")="0.109 kJ K"^(-1)"mol"^(-1)

A liquid is in equilibrium with its vapour at a certain temperature. If deltaH_(vap) = 60.24 kJ mol^(-1) and deltaS_(vap) = 150.6 J mol^(-1) then the boiling point of the liquid will be

The temperature in K at which DeltaG=0 for a given reaction with DeltaH=-20.5 kJ mol^(-1) and DeltaS=-50.0 JK^(-1) mol^(-1) is

A liquid is in equilibrium with its vapour at a certain temperature. If DeltaH_(vap) = 60.24 kJ mol^-1 and DeltaS_(vap) = 150.6 J mol^-1 then the boiling point of the liquid will be

Calculate the change of entropy for the process , water (liq) to water (vapor,373) involving DeltaH_("vap")=40850 J mol ^(-1) " at " 373K.

Calculate the entropy change for vaporization of 1mol of liquid water to stem at 100^(@)C , if Delta_(V)H = 40.8 kJ mol^(-1) .