If `N_2` gas is bubbled through the water is 293K, how many millimoles of `N_2` gas would dissolve in 1 litre of water. Assume that `N_2` exerts a partial pressure of 0.987 bar. The `K_H` for `N_2` at 293K is 76.48 K bar.

If N_2 gas is bubbled through water at 293 K, how many millimoles of N_2 gas would dissolve in 1 litre of water? Assume that N_2 exerts a partial pressure of 0.987 bar. Given that Henry's law constant for N_2 at 293 K is 76.48 kbar.

When a gas is bubbled through water at 298K, a very dilute solution of the gas is obtained. Henry's law constant for the gas at 298K is 100 kbar. If the gas exerts a partial pressure of 1 bar. The number of millimoles of the gas dissolved in one litre of water is

Calculate the amount of CO_2 dissolved at 4 atm in 1dm^3 of water at 298K. The Henry's law constant for CO_2 at 298K is 1.7 k bar.

Calculate the boiling point of solution when 2 g of Na_2SO_4 (M=142gmol^-1) was dissolved in 50 g of water, assuming Na_2SO_4 undergoes complete ionization. (K_b for water=0.52 K kg mol^-1) .

Determine the osmotic pressure of a solution prepared by dissolving 25 mg of K_2SO_4 in 2 litre of water at 25° C, assuming that it is completely dissociated.

The mole fraction of He gas in a saturated solution at 20^@C is 1.25x10^-6 . Calculate the pressure of He gas above the solution. (k_H of He at 20^@C= 144.98 k bar

If 10^(-4) dm^(3) of water is introduced into a 1.0 dm^(3) flask to 300K how many moles of water are in the vapour phase when equilibrium is established ? (Given vapour pressure of H_(2)O at 300K is 3170Pa R =8.314 JK^(-1) mol^(-1)) .

1 kg of water under a nitrogen pressure of 1 atmosphere dissolves 0.02 gm of nitrogenat 293 k. Calculate Henry' s law constant :

A solution of glucose has been prepared at 298K dissolving 7.2 g of glucose in 100 g of water. k_f water is 1.86Km^-1 and vapour pressure of water at 298K is 0.024 atm. The vapour pressure of the solution at 298K will be