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Question

A gaseous mixture contain 56 grams of N244 grams of CO2 and 16 grams of CH4. The total pressure of the mixture is 720 mm Hg. The partial pressure of CH4 is:


A
180 mm
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B
360 mm
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C
540 mm
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D
720 mm
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Solution

The correct option is B $$180$$ $$mm$$
moles of $$N_{2} = \frac {56} {28} = 2$$
moles of $$CO_{2} =\frac {44} {44} =1$$
moles of $$CH_{4} =\frac {16} {16} =1$$
Total moles of mixture = $$4$$
Mole fraction of methane = $$1: 4$$
$$P_{CH_{4}}=P(\displaystyle \frac{n_{CH_{4}}}{n})$$

Chemistry

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