A 5 litre flask contains 3.5gm of $N_{2}$ , 3g of $H_{2}$ and 8g of $O_{2}$ at 27 $^{\circ}$ C.Find the total pressure exerted by the mixture of these gases.

In a 10 litre vessel, the total pressure of a gaseous mixture containing $H_{2}, N_{2} a n d C O_{2}$ is 9.8 atm, The partial pressures of $H_{2} a n d N_{2}$ are 3.7 and 4.2 atm respectively. Find the partial pressure of $C O_{2}$ .

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The total pressure of a mixture of 8g of oxygen and 14g of nitrogen contained in a 11.2L vessel at 0o C is

The correct option is C 1.5 atm PV=nRT V=11.2 lit, n=1428+832 =12+14=34 P=34×22.4273×30011.2=1.49=1.5atm

The total pressure of a mixture of 8g of oxygen and 14g of nitrogen contained in a 11.2L vessel at $0^{o} C$ is

The correct option is C
1.5 atm

PV=nRT
V=11.2 lit, $n = \frac{14}{28} + \frac{8}{32}$
$= \frac{1}{2} + \frac{1}{4} = \frac{3}{4}$
$P = \frac{3}{4} \times \frac{22.4}{273} \times \frac{300}{11.2} = 1.49 = 1.5 a t m$