State and explain Graham's law of Diffusion.

State and explain Graham's law of Diffusion.

State and explain Graham's law of Diffusion.

Deduce a Charles, law b. Graham's law of diffusion from kinetic gas equation.

From a certain apparatus, the diffusion rate of hydrogen has an average value of 28.7" cm"^(3)s^(-1) . The diffusion of another gas under the same conditions is measured to have an average rate of 7.2" cm"^(3)s^(-1) . Identify the gas. [Hint : Use Graham's law of diffusion : R_(1)//R_(2)=(M_(2)//M_(1))^(1//2) , where R1, R2 are diffusion rates of gases 1 and 2 and M_(1) and M_(2) their respective molecular masses. The law is a simple consequence of kinetic theory.]

From a certain apparatus, the diffusion rate of hydrogen has an average value of 28.7 cm^(3) s^(-1) . The diffusion of another gas under the same conditions is measured to have an average rate of 7.2 cm^(3) s^(-1) . Identify the gas. [Hint : Use Graham's law of diffusion: R_(1)//R_(2) = (M_(2) //M_(1) )^(1//2) , where R_(1), R_(2) , are diffusion rates of gases 1 and 2, and M_(1) and M_(2) their respective molecular masses. The law is a simple consequence of kinetic theory.]

From a certain apparatus, the diffusion rate of hydrogen has an average value of 28.7 cm^(3)s^(-1) . The diffusion of another gas under the same conditions is measured to have an average rate of 7.2 cm^(3)s^(-1) . Identify the gas. [Hint: Use Graham's law of diffusion : R_(1)//R_(2) = (M_(2)//M_(1))^(1//2) , where R_(1), R_(2) are diffusion rates of gases 1 and 2, and M_(1) and M_(2) their respective molecular masses. The law is a simple consequence of kinetic theory.]

A vessel contains helium and methane in 4:1 molar ratio at 20 bar pressure. Due to leakage, the mixture of gases starts effusion. Find the composition of the mixture in the initial stage. (Hint: According to Graham's law of effusion, the rate of effusion of a gas in the mixture r prop Partial pressure sqrt((1)/( "molecular mass"))

A vessel contains helium and methane in 4:1 molar ratio at 20 bar pressure. Due to leakage, the mixture of gases starts effusion. Find the composition of the mixture in the initial stage. (Hint: According to Graham's law of effusion, the rate of effusion of a gas in the mixture r prop "Partial pressure" sqrt((1)/("molecular mass"))

State Ohm's law.