What is the vapour pressure of purewater at `100^@C` temperature?

What is the vapour pressure of pure water at 100^(@)C temperature ?

Two liquids X and Y on mixing form an ideal solution. At 30^@C , the vapour pressure of the solution containing 3 mol of X and 1 mol of Y is 550 mm Hg. But when 4 mol of X and 1 mol of Y are mixed, the vapour pressure of the solution thus formed is 560 mm Hg. What would be the vapour pressure of pure X and Y at this temperature?

The vapour pressure lowering caused by the addition of 100 g of sucrose (molecular mass = 342) to 1000 g of water, if the vapour pressure of pure water at 25^@C is 23.8 mm Hg, is

The vapour pressure of water depends upon

6.0 g of urea (molecular weight=60) was dissolved in 9.9 moles of water. If the vapour pressure of pure water is P^@ , the vapour pressure of solution is :

Calculate (1) the enthalpy change in the fusion of 100 g ice at 0^(@)C temperature and 1 atm pressure pressure (2) the enthalpy change in the vaporisation of 10g water at 100^(@)C temperature and 1 atm pressure. Givenn : Latent heat of ice at 0^(@)C temperature and 1 atm pressure =6.02kJ*mol^(-1) and latent heat of vaporisation of water at 100^(@)C temperature= 40.4kJ*mol^(-1) .

Heat required to vaporise 1 g of water at 100^(@)C and 1 atm is 2.26 kJ. What is the enthalpy of vaporisation of water at this temperature and pressure?

The normal boiling point of diethyl ether is 34.6^(@)C . What will be its vapour pressure at this temperature?

The vapour pressure of water at room temperature is lowered by 5% by dissolving a solute in it, then the approximate molality of solution is

The vapour pressure of pure benzene at a certain temperature is 640 mm of Hg. A non-volatile non-electrolyte solid weighing 2.175 g is added to 39 g of benzene. The vapour pressure of the solution is 600 mm of Hg. What is molecular weight of solid substance?