If `Delta H_("vaporisation")` of substance `X (l)` (molar mass `: 30 g//mol`) is 300 J/g at it's boling point 300 K , then molar entropy change for reversible condensation process is

If DeltaH_("vaporisation") of substance X (l) (molar mass :30 g/mol) is 300 J/g at it's boiling piont 300K, then molar entropy change for reversible conddensation process is

If Delta H_("vaporisation") of (C_(2)H_(5))O(l) is 350 J//g at it's boiling point 300 K, then molar entropy change for condensation process is

A substance has latent heat of vaporisation (at its boiling point 300K) = 3kJ//g . If molar mass of substance is 40, the molar entropy change for condensation process will be:

The enthalpy of vaporisation of a substance is 8400 J mol^(-1) and its boiling point is -173^(@)C . The entropy change for vaporisation is :

4.5g mass of a substance (molar mass = 90g/mol) is dissolved in 250ml solution, the molarity of solution is

The entropy of vaporization of a liquid is 58 J K^(-1) mol^(-1) .If 100 g of its vapour condenses at its boiling point of 123^(@)C , the value of entropy change for the process is (molar mass of the liquid = 58 mol^(-1) ).

For the process H_(2)O(l)hArrH_(2)O(g),DeltaH=40.8kJ*mol^(-1) at the boiling poinit of water. Calculate molar entropy change for vaporisation from liquid phase.

The osmotic pressure of a solution of 3.42 g sugar (molar mass 342) in 500 mL at 300 K will be