Dry air contains 79% `N_2` and 21% `O_2`. Determine the proporiton of `N_2` and `O_2` (in terms of mole fraction) dissolved in water at 1 atm pressure. Henry's law constant for `N_2` and `O_2` in `H_2O` are `8.54xx10^4` atm and `4.56xx10^4` atm respectively.

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

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.

The vapour density of a maxture containing NO_2 and N_2 O_4 is 27.6 . The mole fraction of N_2 O_4 in the mixture is :

Draw structure of P_4O_10 and N_2O_5 .

Density of dry air containing ony N_2 and O_2 is 1.15 g/L at 740 mm of Hg and 300 K . What is % composition of N_2 by mass in the air ?

At 300 K, 40 mL of O_(3)(g) dissolves in 100g of water at 1.0atm . What mass of ozone dissolved in 400g of water at a pressure of 4.0atm at 300 K ?

Give the percentages of O_2 in atmospheric air and alveolar air.

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.

A mixture contains N_(2)O_(4) and NO_(2) in the ratio 2:1 by volume. The vapour density of the mixture is:

The experimental data for decomposition of N_2O_5 2N_2O_5 rarr 4NO_2 + O_2 in gas phase at 318K are given below: What is the rate law?