Calculate the work done when done when `1.0` mol of water at `373K` vaporises against an atmosheric pressure of `1.0atm`. Assume ideal gas behaviour.

Calculate the work done when 1.0 mole water at 373K vaporizes against an atmospheric pressure of 1.0 atmosphere. Assume ideal gas behaviour.

Calculate the work donw when 1.0 mol of water at 100^(@)C vaporises against an atmospheric pressure of 1atm . Assume ideal behaviour and volume of liquid water to be negligible.

Calculate the work done (w) and internal energy change ( DeltaU ), when one mole of water at 100^@C vaporises against an atmospheric pressure of 1 atm assuming ideal gas behaviour. Heat of vapourisation of water at 100^@C is 1020 cal mol^(-1) .

Work done in vaporization of 1 mole of water at 373K against a pressure of 1 atm.is approximately. Assume ideal gas behavior

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.

What is the work done against the atmosphere when 25 grams of water vaprorizes at 373 K against a constant external pressure of 1 atm ? Assume that steam obeys perfect gas law. Given that the molar enthalpy of vaporization is 9.72 kcal//"mole" , what is the change of internal energy in the above process?

What is the work done against the atmosphere when 25 grams of water vaprorizes at 373 K against a constant external pressure of 1 atm ? Assume that steam obeys perfect gas law. Given that the molar enthalpy of vaporization is 9.72 kcal//"mole" , what is the change of internal energy in the above process?

Calculate the work done for the vaporisation of 1 mole of water in calories :-(1 atm, 100^(@)C )