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

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

Enthalpy of vapourisation of liquid water is 41 kJ mol^(-1) at 373 K. The change of internal energy when 1mole water at 373 K is converted to steam at 373 K is

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))

Find the molarity of water in pure water(d=1g mol^-1)