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# Calculate the total pressure in a mixture of 4g $O_2\;and \;2g\;H_2$ confined in a bulb of 1 litre at $0^{\large\circ}C$

$(a)\;23.62atm\qquad(b)\;24.32atm\qquad(c)\;26atm\qquad(d)\;25.215atm$

Given
Mole of $O_2$ in a mixture = $\large\frac{4}{32}$
Mole of $H_2$ in mixture = $\large\frac{2}{2} =1$
Total mole present in mixture = 1+$\large\frac{4}{32} = \large\frac{36}{32}$
Also T = 273 K V = 1 litre
We have PV = nRT
$P\times1 = \large\frac{36}{32}\times0.0821\times273$
P = 25.215 atm