[" Assuming the water vapour to be a perfect "],[" gas.calculate the internal energy change "],[" when "1" mol of water at "100^(@)C" and "1" bar "],[" pressure is converted to ice at "0^(@)C" .Given "],[" the enthalpy of fusion of ice is "6.00kJ" mol "],[" theat capacity of water is "4.2J/g^(@)C]

Assuming the water vapour to be a perfect gas, calculate the internal energy change when 1 mol of water at 100^(@)C and 1 bar pressure is converted to ice at 0^(@)C . Given the enthalpy of fusion of ice is 6.00 kJ "mol"^(- 1) heat capacity of water is 4.2 J//g^(@)C The change take place as follows:

Calculate the work done when 1 mol of water vaporises at 100^(@)C and 1 atm pressure. Assume water vapour behaves like an ideal gas.

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) ).

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) ).

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) ).

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

Calculate the entropy change (DeltaS) when 1 mol of ice at 0^(@)C is converted into water at 0^(@)C . Heat of fusion of ice at 0^(@)C is 1436 cal per mol.

Calculate the entropy change (DeltaS) when 1 mol of ice at 0^(@)C is converted into water at 0^(@)C . Heat of fusion of ice at 0^(@)C is 1436 cal per mol.