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Dalton's Law of Partial Pressures

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Question

Find the total pressure exerted by $1.6 g$ methane and $2.2 g C O_{2}$ contained in a four litre flask at $27^{\circ} C$ :

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Solution

Applying dalton's law of partial pressure, total pressure exerted by both gases must be added to find the total pressure. Using the ideal gas equation for both gases we get,
$P V = (n_{1} + n_{2}) R T$
$P \times 4 (\frac{1.6}{16} + \frac{2.2}{44}) \times 0.0821 \times 300$
$P = 0.9236 a t m$ .

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Similar questions

1.6 g

2.2 g

C O_{2}

27^{o} C

What will be the pressure exerted by a mixture of 3.2 g of methane and 4.4 g of carbon dioxide contained in a $9 d m^{3}$ flask at $27^{\circ} C$ ?

3.2 g

4.4 g

9 {d m}^{3}

27^{o} C

3.2 g

4.4 g

9 {dm}^{3}

27^{\circ} C

R = 8.314 {J K}^{- 1} {mol}^{- 1}

3.2 g

4.4 g

C O_{2}

9 d m^{3}

27 C

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