Henry’s law constant for the molality of methane in benzene at 298 K is `4.27xx10^(5)` mm Hg . Calculate the solubility of methane in benzene at 298 K under 760 mm Hg.

Find the density of methane at 298K and 72cm of Hg pressure

The air is a mixture of a number of gases. The major components are oxygen and nitrogen with approximate proportion of 20% is to 79% by volume at 298 K. The water is in equilibrium with air at a pressure of 10 atm. At 298 K if the Henry’s law constants for oxygen and nitrogen at 298 K are 3.30 xx10^(7) mm and 6.51 xx10^(7) mm respectively, calculate the composition of these gases in water .

Henry's law constant for CO_(2) in water is 1.67xx10^(8) Pa at 298 K. Calculate the quantity of CO_(2) in 500 mL of soda water when packed under 2.5 atm CO_(2) pressure at 298 K.

Vapour pressure of aqueous glucose at 373 K is 750 mm Hg. Calculate the molality of solute present dissovled solution.

The Henry's constant for solubility of N_(2) gas in water at 298K is 1.0xx10^(5) atm. The mole fraction of N_(2) in air is 0.8 . The number of moles of N_(2) from air dissolved in 10 moles of water at 298K and 5 atm pressure is :

Vapour pressure of of water at 293K is 17.535 mm Hg. Calculate the vapour pressure of the solution at 293K when 25g of glucose is dissolved in 450g of water ?

A glass bulb of volume 200 cc is sealed at 27^(@) . If the pressure of the gas inside the bulb is 1.25xx10^(-4)cm of Hg, calculate the number of molecules inside the bulb. (Avagadro's number = 6.0225xx10^(23),R=8.314xx10^(7) erg/mole -K)