IIT/JEE Chemistry Practice #23: Graham's Law of Effusion

Dave explains a problem involving Graham's Law of Effusion, focusing on the equilibrium between diatomic chlorine and chlorine radicals. The video explores how to determine the fraction of chlorine molecules dissociated into radicals by measuring the rate of effusion compared to krypton. Using Graham's Law and equilibrium calculations, the video demonstrates how to solve for the average molar mass of the mixture and determine the proportion of dissociated chlorine molecules.

What is the main focus of the problem discussed in the video?

• Determining the boiling point of chlorine

• Measuring the temperature of the reaction

• Understanding the equilibrium between chlorine molecules and radicals

• Calculating the density of chlorine gas

How does the rate of effusion relate to the molar mass of a gas?

• It is inversely proportional to the molar mass

• It is equal to the molar mass

• It is directly proportional to the molar mass

• It is independent of the molar mass

What is the molar mass of krypton used in the calculations?

• 70

• 84

• 35.5

• 62.42

What is the calculated average molar mass of the chlorine mixture?

• 84

• 35.5

• 70

• 62.42

What is the initial concentration of chlorine molecules in the ICE table setup?

• 0.5

• 2

• 1

• 0

How many chlorine radicals are produced from the dissociation of one chlorine molecule?

• Four

• Three

• Two

• One

What fraction of chlorine molecules have dissociated according to the calculations?

• 0.75

• 0.5

• 0.137

• 0.25