Multiple Choice
A sample of N2O diffuses at a rate of 82.5 mL/s in a diffusion apparatus. What will be the rate of diffusion in mL/s for Br2 in the same apparatus, assuming ideal gas behavior?
7. Gases
Effusion
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If NO and NH3 are allowed to effuse through a porous membrane under identical conditions, the rate of effusion for NH3 will be ________ times that of NO.
A
0.82
B
1.22
C
1.00
D
1.50
Verified step by step guidance1
Understand the concept of effusion: Effusion is the process by which gas molecules escape through a tiny hole into a vacuum. According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of its molar mass.
Identify the molar masses of the gases involved: The molar mass of NO (Nitric Oxide) is approximately 30.01 g/mol, and the molar mass of NH3 (Ammonia) is approximately 17.03 g/mol.
Apply Graham's law of effusion: The formula for Graham's law is \( \frac{\text{Rate of effusion of NH}_3}{\text{Rate of effusion of NO}} = \sqrt{\frac{\text{Molar mass of NO}}{\text{Molar mass of NH}_3}} \).
Substitute the molar masses into the formula: \( \frac{\text{Rate of effusion of NH}_3}{\text{Rate of effusion of NO}} = \sqrt{\frac{30.01}{17.03}} \).
Calculate the square root to find the ratio: This will give you the factor by which the rate of effusion of NH3 is greater than that of NO.
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