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3 years ago

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A gas mixture consists of equal masses of methane (molecular weight 16.0) and argon (atomic weight 40.0). If the partial pressur

e of argon is 200. torr, what is the pressure of methane, in torr

1 answer:

pogonyaev3 years ago

8 0

Answer:

80.11 torr

Explanation:

Hello,

In this case, since the masses are equal, we could assume 1 gram for each gas, which result in the following moles:

$n_{CH_4}=\frac{1g}{16.0g/mol}=0.0625molCH_4 \\n_{Ar}=\frac{1g}{40.0g/mol}=0.025molAr$

Thus, the molar fractions:

$x_{CH_4}=\frac{0.0625}{0.0625+0.025}=0.714\\x_{Ar}=1- x_{CH_4}=1-0.714=0.286$

Thus, the total pressure is:

$p=p_{CH_4}+p_{Ar}\\p=x_{CH_4}p+x_{Ar}p\\p=200torr+0.286p\\p=\frac{200torr}{1-0.286}\\ p=280.11torr$

Hence the pressure of methane:

$p_{CH_4}=280.11torr-200torr=80.11torr$

Best regards.

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The expression for rate of reaction will be :

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