Normal boiling point of water is `373 K`. Vapour pressure of water at `298 K` is `23 mm` enthalpy of vaporisation is `40.656 kJ mol^(-1)` if atmopheric pressure becomes `23 mm`, the water will boil at:

The normal boiling point of water is 373K . Vapour pressure of water at temperature T is 19 mmHg . If enthalpy of vaporization is 40.67 kJ//"mol" , then temperature T would be

What is the vapour pressure of water at 373 K ?

The normal boiling point of watr is 373 K (at 760 mm), vapour pressure of water at 298 K is 23 mm. If entyalpy of vaporization is 40.656 kj//mol.the boiling point of water at 23 mm pressure will be :

The normal boiling point of water is 373 k. Vapour pressure of water at temperature T is 19 mm hg. If enthalpy of vapourization is 40.67 kJ/mol, then temperature T would be (use : log 2 = 0.3, R : 8.3 Jk^(-1)mol^(-1) ):

What happens to boiling point of water at 740 mm pressure ?