Ratio of rate of diffusion of H2 and O2 under identical condition of temperature and pressure will be

The rate of diffusion of gases is given by Graham's law, which states that the rate of diffusion of a gas is inversely proportional to the square root of its molar mass.

The molar mass of H2 (Hydrogen) is approximately 2 g/mol and the molar mass of O2 (Oxygen) is approximately 32 g/mol.

So, the ratio of the rate of diffusion of H2 to O2 under identical conditions of temperature and pressure is given by the square root of the inverse ratio of their molar masses.

This can be calculated as follows:

Ratio = sqrt(Molar mass of O2 / Molar mass of H2) = sqrt(32 / 2) = sqrt(16) = 4

So, the ratio of the rate of diffusion of H2 to O2 under identical conditions of temperature and pressure is 4:1. This means that Hydrogen gas diffuses four times faster than Oxygen gas under the same conditions.