At a given temperature and pressure the rate of diffusion is the highest for the gas
`CO_(2)`
`SO_(2)`
`NO_(2)`
`ClO_(2)`

At a given volume and temperature the pressure of a gas

Assertion: A lighter gas diffuses more rapidly than heavier gas. Reason: At a given temperature and pressure, the rate of diffusion of a gas is inversely proportional to the square root of its density.

At identical temperature and pressure the rate of diffusion of hydrogen gas is 3sqrt3 times that of a hydrocarbon having molecular formula C_(n)H_(2n-n) What is the value of n ? .

At identical temperature and pressure the rate of diffusion of hydrogen gas is 3sqrt3 times that of a hydrocarbon having molecular formula C_(n)H_(2n-n) What is the value of n ? .

At a certain temperature and 2 atm pressure equilibrium constant (K_(p)) is 25 for the reaction SO_(2)(g)+NO_(2)(g)hArrSO_(3)(g)+NO(g) Initially if we take 2 moles of each of the four gases and 2 moles of inert gas, what would be the equilibrium partial pressure of NO_(2) ?

For the diffusion of a gas at pressure P, the rate of diffusion is expressed by

At what temperature will the rate of diffusion of N_(2) be 1.6 times the rate of diffusion of SO_(2) at 27°C?

Under identical conditions of temperature and pressure the ratio of the rates of effusion of O_(2) and CO_(2) gases is given by

If helium and oxygen gas are allowed to escape out of a container containing equal amount of He and O_2 under slmllar conditions of temperature and pressure the ratio of rate of diffusion of O_2 to that of He is

At what temperature, the rate of effusion of N_(2) would be 1.625 times that of SO_(2) at 50^(@)C ?