Question

A sample of gas A has a molar mass of 4 grams while a sample of gas B has a molar mass of 16 grams. Which statement holds true?

Answer 1

Answer: The correct statement is gas A effuses faster than gas B.

Explanation:

To know the rate of effusion of gases, we use Graham's law.

Graham's law states that the rate of effusion of a gas is inversely proportional to the square root of the molar mass of gas. The equation that calculates the rate of effusion of a gas is given by:

$\text{Rate of diffusion}\propto \frac{1}{\sqrt{\text{Molar mass of the gas}}}$

As, rate of effusion is inversely related to the molar mass of the gas, so the gas which have less molar mass will effuse faster than the gas which have more molar mass.

Molar mass of gas A = 4 grams

Molar mass of gas B = 16 grams

Putting values in above equation, we get:

$\frac{Rate_{A}}{Rate_{B}}=\sqrt{\frac{M_{B}}{M_{A}}}$

$\frac{Rate_{A}}{Rate_{B}}=\sqrt{\frac{16}{4}}\\\\\frac{Rate_{A}}{Rate_{B}}=2\\\\Rate_A=2\times Rate_B$

Rate of gas A is 2 times more than rate of Gas B. Hence, the correct statement is gas A effuses faster than gas B.

Answer 2

I believe the closest possible answer to this question are:Gas A effuses faster than gas B.The molar mass is directly proportional to the rate of effusion.Thank you for your question. Please don't hesitate to ask in Brainly your queries