Home
Class 12
CHEMISTRY
The enthalpy of evaporation of water at ...

The enthalpy of evaporation of water at 373 K is `40.67 kJ mol^(-1)`. What will be the enthalpy of evaporation at 353 K and 393 K if average molar heats at constant pressure in this range for water in liquid and vapour states are 75.312 and `33.89 JK^(-1) mol^(-1)` respectively?

Text Solution

Verified by Experts

The correct Answer is:
`%` of `CH_(4) = 74.5%`
`%` of `C_(2)H_(5)=25.5%`
Promotional Banner

Similar Questions

Explore conceptually related problems

The enthalpy of vaporisation of water at 100^(@)C is 40.63 KJ mol^(-1) . The value Delta E for the process would be :-

The enthalpy of vaporisation of a liquid is 30 kJ mol^(-1) and entropy of vaporisation is 75 J mol^(-1) K^(-1) . The boiling point of the liquid at 1atm is :

The enthalpy of vaporisation of a liquid is 30 kJ mol^(-1) and entropy of vaporisation is 75 J mol^(-1) K^(-1) . The boiling point of the liquid at 1atm is :

The enthalpy of vaporisation of a liquid is 30 kJ mol^(-1) and entropy of vaporisation is 75 J mol^(-1) K^(-1) . The boiling point of the liquid at 1atm is :

Standard enthalpy of vapourisation DeltaH^(@) forwater is 40.66 KJ mol^(-1) .The internal energy of vapourisation of water for its 2 mol will be :-

The enthalpy change for transition of liquid water to steam is 40.8 kJ mol^(-1) at 373K. Calculate Delta S for the process.

If the enthalpy of vapourization of a liquid X is 30 kJ/mol and its entropy of Vaporization is 75 Jmol^-1K^-1 the temperature of vapours of liquid X at 1 atmosphere pressure is nearly

The enthalpy of vaporization of liquid is 40 kJ mol^(−1) and entropy of vaporization is 64 J mol^(−1)k^(−1) . The boiling point of the liquid is

If the entropy of vaporisation of a liquid is 110 JK^(-1)mol^(-1) and its enthalpy of vaporisation is 50 kJ mol^(-1) . The boiling point of the liquid is

The heat of combustion of H_(2)(g) at constant pressure and 300k is -280kJ mol^(-1) . What will be the heat of combustion at constant volume and at 300K ?