Calculatte the molal elevation constant of water if molar enthalpy of vapourisation of water at 373K is 40.585 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) ).

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) ).

A glass vassel after washing contain 54 g of water in it. How much heat must be supplied to evaporate this water? Standard enthalpy of vapourisation of water is 40.79 kJ mol^-1 .

Calculate the value of molal elevation constant for water if Delta S_("vaporisation") is 26.33 cal K^(-1) mol^(-1) .

DeltaH (vap) for water is 40.7 kJ mol^(-1) . The entropy of vapourisation of water is

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