What gas law states "Under the same conditions of temperature and pressure, the rates of diffusion for gases are inversely proportional to the square roots of the their molar masses in g/mol".
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At a given temperature and pressure the rate of diffusion of a gas is (1) Directly proportional to the density of the gas (2) Directly proportional to the square root of its density (3) Inversely proportional to the density of the gas (4) Inversely proportional to the square root of its density
Charles's law states that: Equal amounts of gases occupy the same volume at constant temperature and pressure. The rates of effusion of gases are inversely proportional to the square roots of their molar masses. The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature. The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure. The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.
Adi S.
At constant volume and temperature conditions, the rates of diffusion $\mathrm{D}_{A}$ and $\mathrm{D}_{\mathrm{B}}$ of gases $\mathrm{A}$ and $\mathrm{B}$ having densities $\rho_{A}$ and $\rho_{n}$ are related by the expression (a) $\mathrm{D}_{\mathrm{A}}=\left[\mathrm{D}_{\mathrm{a}} \rho_{\mathrm{A}} / \rho_{\mathrm{h}}\right]^{1 / 2}$ (b) $\mathrm{D}_{\mathrm{A}}=\left[\mathrm{D}_{\mathrm{B}} \rho_{\mathrm{B}} / \rho_{A}\right]^{1 / 2}$ (c) $D_{A}=D_{B}\left[\rho_{A} / \rho_{B}\right]^{1 / 2}$ (d) $\mathrm{D}_{\mathrm{A}}=\mathrm{D}_{\mathrm{B}}\left[\rho_{\mathrm{B}} / \rho_{\mathrm{A}}\right]^{12}$
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