Under the same conditions of temperature and pressure, the rate of diffusion of hydrogen gas is four times that of oxygen gas-explain.

Explanation

At constant temperature and pressure, rates of diffusion (r) of different gases are inversely proportional to the square roots of their molecular masses (M) i.e., `r prop (1)/(sqrt(M))`
Undre identical conditions of temperature and pressure, if the rates of diffusion of `H_(2) and O_(2)` are `r_(H_(2))` and `r_(O_(2))` respectively, then `(r_(H_(2)))/(r_(O_(2)))=(sqrt(M_(O_(2))))/(sqrt(M_(H_(2))))=(sqrt(32))/(sqrt(2))=4 or, r_(H_(2))=4xxr_(O_(2))`
So, under the same conditoins of temperature and pressure, rate of diffusion of `H_(2)` gas is four times that of `O_(2)` gas.