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One mole of nitrogen gas at 0.8atm takes...

One mole of nitrogen gas at `0.8atm` takes `38s` to diffuse through a pinhole, while `1 mol` of an unknown fluoride of xenon at `1.6 atm` takes `57 s` to diffuse through the same hole. Calculate the molecular formation of the compound.

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To solve the problem, we will use Graham's law of effusion, which states that the rate of diffusion of a gas is inversely proportional to the square root of its molar mass. The formula can be expressed as: \[ \frac{R_1}{R_2} = \frac{P_1}{P_2} \cdot \frac{\sqrt{M_2}}{\sqrt{M_1}} \] Where: - \( R_1 \) and \( R_2 \) are the rates of diffusion of gas 1 and gas 2, respectively. ...
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One mole of nitrogen gas at 0.8atm takes 38s to diffuse through a pinhole, while 1 mol of an unknown fluoride of xenon at 1.6 atm takes 57 s to diffuse through the same hole. Calculate the value of n in the compound if formula is XeF_n .

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