A gaseous mixture of three gases A, B and C has a pressure of 10atm. The total number of moles of all gases is 10. The partial pressure of A and B are 3 and 1 atm respectively. If C has a molecular weight of 2, then find the weight of C in grams present in the mixture.

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3 grams of H2 and 24 grams of O2 are present in a gaseous mixture at constant temperature and pressure. The partial pressure of H2 is:

The correct option is B 23 of total pressureNo. of moles of H2=32=1.5No. of moles of O2=2432=3:4=0.75PH2=(nH2nH2+nO2)× total pressurePH2=23 of total pressure

3 grams of $H_{2}$ and 24 grams of $O_{2}$ are present in a gaseous mixture at constant temperature and pressure. The partial pressure of $H_{2}$ is:

The correct option is B $\frac{2}{3}$ of total pressure
No. of moles of $H_{2} = \frac{3}{2} = 1.5$

No. of moles of $O_{2} = \frac{24}{32} = 3 : 4 = 0.75$

$P_{H_{2}} = (\frac{n_{H_{2}}}{n_{H_{2}} + n_{O_{2}}}$ ) $\times$ total pressure

$P_{H_{2}} = \frac{2}{3}$ of total pressure