In a 10 litre volumetric flask contains 1 gram He and 6.4 gram `O_(2)` at `27^(@) C` temperature . If that total pressure of the mixture is 1.107 atmosphere , then what is the partial pressure of `He` and `O_(2)` ?

In a 10 litre volumetric flask contains 1 gram He and 6.4 and gram O_2 at 27^@C temperature If that total pressure of the mixture is 1.107 atmosphere then what is the partial pressure of He and O_2 ?

(i) For which property of the liquid the shape of a liquid drop is spherical? (ii) In a 10 volumetric flask contains 1 g He and 6.4 g of O_(2) at 27^(@)C temperature. If the total pressure of the mixture is 1.107 atm, then what is the partial pressure of He and O_(2) ?

A 2L flask contains 0.4 g O_(2) and 0.6 g H_(2) at 100^(@)C . Calculate the total pressure of the gas mixture in the flask.

A mixture of O_(2) and H_(2) gases contains 20% of H_(2) gas. At a certain temperature, the total pressure of the mixture is found to be 1 bar. What is the partial pressure of O_(2) (in bar) in the mixture?

At 100^(@)C a 2 litre flask contains 0.4 g of O_(2) and 0.6 g of H_(2) . What is the total pressure of this gas mixture in the flask?

What is partial pressure? If the total pressure of a mixture of 4 gm H_2 & 16 gm O_2 at 27^@C be 5 atm. find the ratio of partial pressure . of H_2 & O_2

At 27^(@)C , a cylinder of volume 10 L contains a gas mixture consisting of 0.4 He, 1.6g O_(2)&1.4g H_(2) . Determine the total pressure of the mixture and the partial pressure of He in the mixture.

A gas mixture was prepared by taking equal mole of CO and N_(2) . If total pressure of the mixture was 1 atm, the partial pressure of N_(2) in the mixture is-

A vessel contains equal masses of CH_(4) and H_(2) gas at 25^(@)C . What part of the total pressure inside the vessel is equal to the partial pressure of H_(2) gas?