Assuming that water vapour is an ideal gas, the internal energy change `(DeltaU)` when 1 mole of water is vaporised at 1 bar pressure and `100^(@)C` , (given: molar enthalpy of vaporisation of water `-41KJmol^(-1)` at 1 bar and `373K` and `R=8.3Jmol^(-1)Kmol^(-1)`) will be:

Assuming that water vapour is an ideal gas, the internal energy change (DeltaU) when 1 mole of water is vaporised at 1 ba r pressure and 100^(@)C, ( given : molar enthalpy of vaporization of water 41kJ mol^(-1) at 1 ba r and 373 K and R=8.3 J mol^(-1)K^(-1)) will be :

Assuming that water vapour is an ideal gas, the internal energy change (Delta U) when 1 mol of water is vapourised at 1 bar pressure and 100^(@)C , (Given: Molar enthalpy of vapourization of water at 1 bar and 373K=41 kJ mol^(-1) and R=8.3J mol^(-1)K^(-1) ) will be:

Assuming that water vapour is an ideal gas, the internal energy change (DeltaU) when 1 mol of water is vapourised at vapourisation of water at 1 bar and 373K=41 kJmol^-1 and R=8.3 Jmol^-1K^-1 will be

90 g of water spilled out from a vessel in the room on the floor. Assuming that water vapour behaving as an ideal gas, calculate the internal energy change when the spilled water undergoes complete evaporation at 100^(@)C . (Given the molar enthalpy of vaporisation of water at 1 bar and 373 K = 41 kJ mol^(-1) ).

Entropy of vaporisation of water at 100^(@)C , if molar heat of vaporisation is 9710 cal mol^(-1) will be