A mixture of 4 gm of hydrogen and 16 gm of oxygen has a total pressure, of 750 mm. Calculate the partial pressure of oxygen.

A mixture of hydrogen and oxygen at one bar pressure contains 20% by weight of hydrogen. Calculate partial pressure of hydrogen.

A mixture of dihydrogen and dioxygenn at oone bar pressure contains 20% by weight of dihydrogen. Calculate the partial pressure of dihydrogen.

Assuming that the air is essentially a mixture of nitrogen and oxygen in mole ratio of 4 : 1 by volume. Calculate the partial pressures of N_2 and O_2 on a day when the atmospheric pressure is 750 mm of Hg. Neglect the pressure of other gases.

Calculate the total pressure in a 10 L cylinder which contains 0.4 g of helium, 1.6 g of oxygen and 1.4 g of nitrogen at 27^(@) C. Also calculate the partial pressures of He gas in the cylinder. Assume Ideal behaviour for gases. R = 0.082 L atm k^(-1) mol^(-1)

A mixture of N_(2) and O_(2) at 1 bar pressure contains 80% N_(2) by weight. Calculate the partial pressure of N_(2) in the mixture.

A gaseous mixture was prepared by taking equal moles of CO and N_2 . If the total pressure of the mixture was found 1 atm, the partial pressure of the nitrogen (N_2) in the mixture is

A gaseous mixture contains three gases A, B and C with a total number of moles of 10 and total pressure of 10 atm. The partial pressures of A and B are 3 atm and 1 atm respectively and if C has molecular weight of 2. Then, the weight of C present in the mixture will be

the partial pressure of oxygen in the alveolar air is

Calculate the number of moles of 32 gm of oxygen gas.