Bromine boils at `59^(@)C` with `DeltaH_(vap)^(@)=29.6kJ mol^(-1)` What is the value of `DeltaS_(vap)^(@)"in"29.6 J mol^(-1)K^(-1)`

If Delta H_("vap") of pure water at 100^(@)C is 40.627 kJ mol^(-1) . The value of Delta S_("vap") is

A reaction is at equilibrium at 100^(@)C and the enthalpy change for the reaction is "42.6 kJ mol"^(-1) . What will be the value of DeltaS in "J K"^(-1)"mol"^(-1) ?

A reaction is at equilibrium at 100^(@)C and the enthalpy change for the reaction is "42.6 kJ mol"^(-1) . What will be the value of DeltaS in "J K"^(-1)"mol"^(-1) ?

For a substance with the value of DeltaH_(vap) and DeltaS_(vap) given below, what is its normal boiling point in .^(@)C (DeltaH_(vap)=59.0 kJ mol^(-1), DeltaS_(vap)=93.65 Jmol^(-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)

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)

Chloroform has DeltaH_("vaporization")=29.2 kJ//"mol" and boils at 61.2^(@)C . What is the value of DeltaH_("vaporization")=29.2 kJ//"mol" for chloroform ?

Chloroform has DeltaH_("vaporization")=29.2 kJ//"mol" and boils at 61.2^(@)C . What is the value of DeltaS_("vaporization") for chloroform ?

Chloroform has DeltaH_("vaporization")=29.2 kJ//"mol" and boils at 61.2^(@)C . What is the value of Delta S _ ("vaporization") for chloroform ?