A) The average molecular speed in a sample of Ar gas at a certain temperature is 391 m/s. The average molecular speed in a sample of Ne gas is m/s at the same temperature. B) The rate of effusion of Xe gas through a porous barrier is observed to be 7.03×10-4 mol / h. Under the same conditions, the rate of effusion of SO2 gas would be mol / h

For A: The average molecular speed of Ne gas is 553 m/s at the same temperature.

For B: The rate of effusion of gas is

Explanation:

For A:

The average molecular speed of the gas is calculated by using the formula:

     OR

where, M is the molar mass of gas

Forming an equation for the two gases:

         .....(1)

Given values:

Plugging values in equation 1:

Hence, the average molecular speed of Ne gas is 553 m/s at the same temperature.

For B:

Graham's law states that the rate of diffusion of a gas is inversely proportional to the square root of the molar mass of the gas. The equation for this follows:

Where, M is the molar mass of the gas

Forming an equation for the two gases:

         .....(2)

Given values:

Plugging values in equation 2:

Hence, the rate of effusion of gas is

93.2 ml + 3920 ml = 4013 ml total  

(93.2 ml) * (2.03 m) / (4013 ml) = 0.0471 m

the volume in in l of the diluted solution would be 0.0471 m.

its going to be mutualism cuz they both benefit from the relationship.

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