Which of the following would effuse at a rate equal to 31.5% of the rate of H2?COHCNCOCl2NeNH3

The question is asking which of the given gases would effuse at a rate that is 31.5% of the rate of Hydrogen gas (H2).

This is a question about Graham's Law of Effusion, which states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass.

The formula for Graham's Law of Effusion is:

Rate1/Rate2 = sqrt(M2/M1)

Where: Rate1 is the rate of effusion of gas 1 (in this case, H2) Rate2 is the rate of effusion of gas 2 (the gas we're trying to find) M1 is the molar mass of gas 1 (H2) M2 is the molar mass of gas 2

We know that the rate of effusion of the unknown gas is 31.5% of the rate of H2, so we can set up the equation as follows:

0.315 = sqrt(M2/2.016)

Squaring both sides to get rid of the square root gives:

0.099225 = M2/2.016

Solving for M2 gives:

M2 = 0.099225 * 2.016 = 0.2 g/mol

Looking at the molar masses of the given gases, the one that is closest to 0.2 g/mol is Ne (Neon), with a molar mass of 20.18 g/mol.

Therefore, Ne (Neon) would effuse at a rate equal to 31.5% of the rate of H2.