Home
Class 12
CHEMISTRY
Calculate the entropy increase in the ev...

Calculate the entropy increase in the evaporation of 1 mole of a liquid when it boils at `100^@C` having heat of vaporisation at `100^@C` as 540 cals\gm.

Text Solution

Verified by Experts

`Delta S = 26.06 cal K^(-1) mol^(-1)`
Promotional Banner

Similar Questions

Explore conceptually related problems

Calculate the entropy change involved in convertion of 1 mole of water at 373 K to vapours at the same temperature. Latent heat of vaporisation of water = 2.257 kJ g^(-1) .

Calculate the vapour pressure of an aqueous solution of 1.0 molal glucose solution at 100^(@)C .

Define entropy.Calculate entropy change for the following reversible process : 1 mole of liquid water at 1 atm 100^@C evaporates to 1 mole water vapours (Delta_vap for H_2O=2257 jg^-1)

The enthalpy of vaporisation of a compound AB a its boiling point (127^(@)C) is 6.4 kJ mol^(-1) . Its entropy of vapourisation is :

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 :

The boiling point of 0.1 M KCl solution is ………..than 100^(@)C .

What is the entropy change of an engine that operates at 100^@C when 453.6 k.cal of heat is supplied to it?

Calculate the molar mass of a substance 1 g of which when dissolved in 100 g of water gave a solution boiling at 100.1^(@)C at a pressure of 1 atm (K_(b) for water = 0.52 K kg mol^(-1))