A mixture of gases at 2.99 atm can You have two gases, and , at the same temperature. Determine the ratio of effusion rates of and .ists of

Question

A mixture of gases at 2.99 atm can You have two gases, and , at the same temperature. Determine the ratio of effusion rates of and .ists of 13.2 moles of hydrogen gas and 19.1 moles of helium gas. Determine the partial pressure of the helium gas.

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bonexptip 6 months 2021-07-17T06:55:41+00:00 1 Answers 14 views 0

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    2021-07-17T06:56:56+00:00

    Answer:

    Given total pressure of the gas mixture(hydrogen and helium) is 2.99 atm

    Number of moles of hydrogen is —- 13.2 mol

    Number of moles of helium is —- 19.1 mol

    Determine the partial pressure of the helium gas.

    Ratio of effusion rates of the two gases.

    Explanation:

    According to Dalton’s law of partial pressures,

    partial pressure of a component gas in a mixture is:

    partial pressure of a gas = total pressure x mole fraction

    mole fraction of helium gas is:

    mole fraction of helium gas = \frac{number of moles of helium gas}{total number of mioles} \\=>mole fraction of He= \frac{19.1mol}{(19.1+13.2)mol} \\=>mole fraction of He = 0.591\\

    Partial pressure of He gas is:

    Partial pressure of He =mole fraction of He * total pressure\\                                      =0.591 x 2.99atm\\                                      =1.77atm

    Effusion rate of a gas is inversely proportional to its square root of its molecular mass.

    \frac{rate of effusion of H2 gas}{rate of effusion of He gas} =\sqrt{\frac{molar mass of He gas}{molar mass of H2 gas} } \\=> \frac{rate of effusion of H2 gas}{rate of effusion of He gas}=\sqrt{\frac{4g.}{2g} } \\=>\frac{rate of effusion of H2 gas}{rate of effusion of He gas}=1.414:1

    Hence, rates of effusion of H2:He is 1.414:1.

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