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Gay Lussac's Law

The pressure ...

Question

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 $27^{o} C$ 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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Solution

$Volume, V = 10 L Temperature, T = 27^{o} C = 300 K$
$M a s s {(m)}_{m e t h a n e} = 6.4 g M a s s (m)_{C O_{2}} = 8.8 g$
$Mole of methane = \frac{6.4}{16} = 0.4 m o l$
$Mole of carbon dioxide = \frac{8.8}{44} = 0.2 m o l$
$P V = n_{t o t a l} R T$

$P \times 10^{- 2} = (0.4 + 0.2) \times 8.314 \times 300$

$P = 149652 P a \Rightarrow P = 149.652 k P a \approx 150 k P a$

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