Graham's Law of Diffusion

Two gases A and B having the same volume diffuse through a porous partition in 20 and 10 seconds respectively. The molecular mass of A is 49 u. Molecular mass of B will be:

From a heated mixture of nitrogen, oxygen and carbon, two compounds (out of the many obtained) are isolated. The rates of diffusion of the two isolated compounds are almost identical. The two compounds are

Two gases A and B are kept in two cylinders and allowed to diffuse through a small hole. If the time taken by gas A is four times the time taken by gas B for diffusion of equal volume of gas under similar conditions of temperature and pressure, what will be the ratio of their molecular masses?

A cylinder is filled with a mixture of equal number of molecules of oxygen, carbon dioxide and helium. When leakage occurs, do equal amounts of gases come out? Give a reason.

$500 \mathrm{mL}$ of a mono atomic gas X diffuses through a hole at a pressure of $4 \mathrm{atm}$ and $127°\mathrm{C}$. $1500 \mathrm{mL}$ of another elemental diatomic gas Y diffuses through the same hole at pressure of $2 \mathrm{atm}$ and $27°\mathrm{C}$. If the time taken for both the diffusion process is same, then compare the atomic weights of the two gases.

The ratio of rates of diffusion of two gases X and Y is $4 : \sqrt{11}$. If the molecular mass of Y is double to the molecular mass of oxygen, then X is:

If equal volumes of two gases, ${\mathrm{CH}}_4$ and ${\mathrm{O}}_2$, are allowed to diffuse, then the time taken for diffusion of ${\mathrm{CH}}_4$ is found to be:

Under similar conditions of temperature and pressure the ratio of rate of diffusion of methane and sulphur dioxide is $2 : 1$.

The rate of diffusion of two gases $\mathrm{A} \& \mathrm{B}$ at same volume are $8$ and $12 \mathrm{m}/\mathrm{s}$ respectively. If gas $\mathrm{A}$ hass molecular weight is $81 \mathrm{g}/\mathrm{mol}$, so what will be the molecular weight of gas$\mathrm{B}$ ?

A balloon filled with helium is pierced with a needle and quickly dropped in a tank of hydrogen gas under identical conditions, the balloon will

Equal volumes of two gases $\mathrm{A}$ and $\mathrm{B}$ diffuse through a porous pot in $20$ and $10$ seconds respectively. If the molar mass of $\mathrm{A}$ is $80$, calculate the molar mass of $\mathrm{B}$.

Through the two ends of a glass tube of length $200 \mathrm{cm}$, hydrogen chloride gas $\left(\mathrm{HCl}\right)$ and ammonia $\left({\mathrm{NH}}_3\right)$ are allowed to enter. At what distance ammonium chloride will first appear ?

State the Graham's law of diffusion and derive the equation to calculate molecular masses of unknown gases.

State Graham's law of diffusion. Write any two applications of Graham's law of diffusion. 

Select the correct statement according to Graham's law of diffusion.

The time taken for a certain volume of gas to diffuse through a small hole was $2 \min$. Under similar conditions an equal volume of oxygen took $5.65$ minute to pass. The molecular mass of the gas is

$100 \mathrm{mL}$ of ${\mathrm{O}}_2$ gas diffuses in $10 \mathrm{s}$. $100 \mathrm{mL}$ of gas${\mathrm{X}}^{\text{'}}$ diffuses in ' $\mathrm{t}$ ' second. Gas ' $\mathrm{X}$ ' and time ' $\mathrm{t}$ ' can be

The rates of diffusion of gases $\mathrm{A}$ and $\mathrm{B}$ of molecular weights $100$ and $81$ respectively are in the ratio of

At STP $16 \mathrm{mL}$ of ${\mathrm{O}}_2$ diffused through a porous partition in t seconds. What volume of ${\mathrm{CO}}_2$ will diffuse in the same time and under the same conditions?

If two molecules of $\mathrm{A}$ and $\mathrm{B}$ having mass $100 \mathrm{Kg}$ and $64 \mathrm{Kg}$ and rate of diffusion of $\mathrm{A}$ is $12\times {10}^{-3}$, then rate of diffusion of $\mathrm{B}$ will be