The pressure exerted by a non-reactive gaseous mixture of 6.4 g of methane and 8.8 g of carbon dioxide in a 10 L vessel at 27°C is _____kPa.
(Round off to the Nearest Integer).[Assume gases are ideal, $R = 8.314 J m o l^{- 1} K^{- 1}$ ,Atomic masses: C:12.0 u, H:1.0 u, O:16.0 u]

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answer is 150.

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Detailed Solution

$\begin{array}{l} n_{{CH}_{4}} = \frac{6 .4}{16} = 0 .4 n_{{CO}_{2}} = \frac{8 .8}{44} = 0 .2 n = 0 .6 \\ PV = nRT P \times 10 \times 10^{- 3} = 0 .6 \times 8 .314 \times 300 \\ = 149 .652 kpa ≃ 150 kpa \end{array}$

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