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Ideal Gas Equation

What will be ...

Question

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

0.82 a t m

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8.314 \times 10^{4} a t m

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1 a t m

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1.8 a t m

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Solution

The correct option is B $0.82 a t m$
From Ideal gas law-
$P = \frac{n}{V} R T$

$n$ for $C H_{4} = \frac{3.2}{16} = 0.2;$

$n$ for $C O_{2} = \frac{4.4}{44} = 0.1$

$n_{t o t a l} = 0.2 + 0.1 = 0.3$

$P = \frac{0.3 \times 0.0821 \times 300}{9} = 0.82 a t m$ .

Hence, option A is correct.

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Similar questions

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

C O_{2}

9 d m^{3}

27 C

3.2 g

4.4 g

9 {dm}^{3}

27^{\circ} C

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

3.2 g

0.2 g

1.12 l i t r e

0^{\circ} C

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