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Dalton's Law of Partial Pressures

A vessel has ...

Question

A vessel has a mixture of $O_{2}$ and $N_{2}$ . What will be the ratio in their partial pressure if their masses are the same?

A

0.875 : 1

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B

1 : 1.15

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C

2.03 : 1

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D

3.75 : 1

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Solution

The correct option is A $0.875 : 1$
In a vessel mixture of $O_{2}$ & $N_{2}$ are present.
Molecular weight of oxygen $= 16$ $(\frac{14}{16} = \frac{0.875}{1})$
Molecular weight of Nitrogen $= 14$
Partial pressure of oxygen $= 0.875 \times$ Partial pressure of Nitrogen.
$P (O_{2}) : P (N_{2}) = 0.875 : 1$

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