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)`

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)

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)

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) .

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

Delta_(vap)H = 30 kJ mol^(-1) and Delta_(vap)S = 75 mol^(-1)K^(-1) . Find the temperature of vapour, at 1 atm.

Delta_(vap)H = 30 kJ mol^(-1) and Delta_(vap)S = 75Jmol^(-1)K^(-1) . Find the temperature of vapour, at 1 atm.