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Dalton's Law of Partial Pressures

A closed bulb...

Question

A closed bulb capacity 200ml containing ${C H}_{4}$ , $H_{2}$ and He at 300K. The ratio of partial pressure of ${C H}_{4}$ , $H_{2}$ and He, respectively is 2:3:5. Calculate the ratio of their weights present in the container.

A

2:4:6

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B

16:8:100

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C

16:3:10

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D

4:9:25

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Solution

The correct option is C 16:3:10
Partial pressure $=$ mole fraction $\times$ total pressure
$∴$ Mass are also in $2 : 3 : 5$

$∴$ Ratio of mass $= 2 \times 16 : 3 \times 2 : 5 \times 4$
$= 16 : 3 : 10$

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