Write equilibrium constant in terms of partial pressure and molar concentration. Why vaporisation of water takes place rapidly at low pressure and high temperature.

Using van der waals equation, explain why real gases behave like an ideal gas at very low pressures and high temperature.

Water remains in equilibrium with its vapour at 100^(@)C and 1 atm. Will the transformation of water into its vapour be spontaneous at this pressure and temperature?

It the free energy change for a reaction at 25^@C be 5.4 Kj Calculate the equilibrium constant for the reaction. State wheather the vaporisation of water at 110^@C in 1 atm pressure is a spontaneous or non spontaneous process.

At a given temperature and pressure, the enthalpies of condensation and vaporisation for a given liquid, are the same but opposite in sign. Why?

Why does not the equilibrium constant expression for a reaction involving pure solids or liquid contain the concentrations terms of the solid or liquids?

At 540, the equilibrium constant K_(p) for PCl_(5) dissociation equilibrium at 1.0 atm 1.77 atm. Calculate equilibrium constant in molar concentration (K_(c)) at same temperature and pressure.

Calculate the values of Delta H and DeltaU in the vaporisation of 90g of water at 100^(@)C and 1 atm pressure. The latent heat of vaporisation of water at the same temperature and pressure =540cal*g^(-1)

Calculate (1) the enthalpy change in the fusion of 100 g ice at 0^(@)C temperature and 1 atm pressure pressure (2) the enthalpy change in the vaporisation of 10g water at 100^(@)C temperature and 1 atm pressure. Givenn : Latent heat of ice at 0^(@)C temperature and 1 atm pressure =6.02kJ*mol^(-1) and latent heat of vaporisation of water at 100^(@)C temperature= 40.4kJ*mol^(-1) .

Write the relation between the pressure and density of a gass at a constant temperature.

Write the relationship between the pressure and density of a gas at a constant temperature.