The enthalpy change for the conversion of liquid water to steat is '40.8 k J' at '100^circ C'. Calculate 'Delta S' for the process.

The enthalpy change for the evaporation of a liquid at its boiling point 127^(@)C is + 40.32 k J mol^(-1) . What is the volume of internal energy change for the above process at 127^(@)C ? (R = 8.3 JK^(-1) mol^(-1))

Calculate the enthalpy change on freezing of '1.0 mol' of water at '10.0^circ C' to ice at '-10.0^circ C . Delta_( fus) H=6.03 kJ mol^(-1)' at '0^circ C .' 'C_p[H_2 O(t)]=7 5 . 3 J m o l^(-1) K^(-1)' 'C_p[H_2 O(s)]=36.8 J mol^(-1) K^(-1)'

Molar enthalpy change for vapourisation of 1 mol of water at 100^@C and 1 bar pressure is 41 kJ mol^-1 . Assuming water vapour to be a perfect gas, calculate the internal energy change when (i) 1 mol of water is vapourised at 1 bar pressure and 100^@C

Molar enthalpy change for vapourisation of 1 mol of water at 100^@C and 1 bar pressure is 41 kJ mol^-1 . Assuming water vapour to be a perfect gas, calculate the internal energy change when (ii) 1 mol of water is converted to ice