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Dalton's Law of Partial Pressures

In a gaseous ...

Question

In a gaseous mixture at $20^{o} C$ the partial pressure of the components are
$H_{2} : 150$ Torr ${C H}_{4} : 300$ Torr
${C O}_{2} : 200$ Torr $C_{2} H_{4} : 100$ Torr
Volume percent of $H_{2}$ is:

A

26.67

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B

73.33

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C

80.00

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D

20

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Solution

The correct option is D $20$
In a mixture of gases the percent of each gas in the volume is same as the percent of each partial pressure in the total pressure.
Total partial pressure= $150 + 300 + 200 + 100 = 750$ torr
$v o l u m e p e r c e n t H 2 = \frac{150}{750} \times 100 = 20$

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