Lowering of vapour pressure due to a solute in `1` molal aqueous solution at `100^(@)C` is
a.`13.44 mm Hg` ,b. `14.14 mm Hg` ,c.`13.2 mm Hg` ,d. `35.2 mm Hg`

The vapoure pressure of an aqueous solution of glucose is 750 mm of Hg at 373 K. the molality is

What will be the relative lowering in vapour pressure when 1 mole of A(l) is dissolved in 9 moles of B(l). Given both are volatile with vapour pressures as 100 mm of Hg and 300 mm of Hg respectively?

The total vapour pressure of a mixture of 1 mole of A ( P_A = 200 mm Hg ) and 3 mole of B ( P_B= 360 mm Hg) is 350 mm Hg. Then

The vapour pressure of a dilute aqueous solution of glucose is 750 mm Hg at solution of glucose is 750 mm Hg at 373 K. The mole fraction of the solute is ______.

The vapour pressure of an aqueous solution of glucose is 750 mm of Hg at 373 K . Calculate molality and mole fraction of solute.

At 25^(@)C , the vapour pressure of pure water is 25.0 mm Hg . And that of an aqueous dilute solution of urea is 20 mm Hg . Calculate the molality of the solution.

At 25^(@)C , the vapour pressure of pure water is 25.0 mm Hg . And that of an aqueous dilute solution of urea is 20 mm Hg . Calculate the molality of the solution.

At 25^(@)C , the vapour pressure of pure water is 25.0 mm Hg . And that of an aqueous dilute solution of urea is 20 mm Hg . Calculate the molality of the solution.

If at certain temperature, the vapour pressure of pure water is 25 mm Hg and that of a very dilute aqueous urea solution is 24.5 mm Hg, the molality of the solution is