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Standard XII

Chemistry

Concentration Terms

The density o...

Question

The density of a mixture of $O_{2}$ and $N_{2}$ at NTP is 1.3 g litre $^{- 1}$ . Calculate partial pressure of $O_{2}$ .

0.28 atm

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0.30 atm

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0.56 atm

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0.12 atm

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Solution

The correct option is A 0.28 atm
Density $= \frac{Weight}{Volume}$
At S.T.P., $1.3 = \frac{Weight}{22.4} \Rightarrow Weight = 22.4 \times 1.3 = 29.12 g$

Weight $_{m i x t u r e} = 29.12 =$ Weight $_{O_{2}} +$ Weight $_{N_{2}} = n_{O_{2}} M_{O_{2}} + n_{N_{2}} M_{N_{2}} = x \times 32 + (1 - x) \times 28$
$x = 0.28 m o l e$
(where n represents the molecular weight and x represents mole fraction)
Moles of $O_{2} = 0.28$
At S.T.P., pressure $= 1 a t m$
Partial pressure of $O_{2} = \frac{n_{O_{2}}}{n_{t o t a l}} \times p r e s s u r e = \frac{0.28}{1} \times 1 = 0.28$ atm.

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The density of a mixture of O2 and N2 at NTP is 1.3 g litre−1. Calculate partial pressure of O2.

The density of a mixture of $O_{2}$ and $N_{2}$ at NTP is 1.3 g litre $^{- 1}$ . Calculate partial pressure of $O_{2}$ .