You visited us 1 times! Enjoying our articles? Unlock Full Access!

Ideal Gas Equation

Find the tota...

Question

Find the total pressure exerted by $1.6 g$ of methane and $2.2 g$ of $C O_{2}$ contained in a four-litre flask at $27^{o} C$ .

Open in App

Solution

$n_{C H_{4}} = \frac{1.6}{16} = 0.1, n_{C O_{2}} = \frac{2.2}{44} = 0.05$

$n_{C H_{4}} + n_{C O_{2}} = 0.15$

$V = 4 l i t, T = 273 + 27 = 300 K$ .

$\Rightarrow P V = n R T$

$\Rightarrow P = \frac{n R T}{V} = \frac{0.15 \times 0.0821 \times 300}{4} = 0.924 a t m$

Suggest Corrections

Similar questions

1.6 g

2.2 g C O_{2}

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

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 $27^{\circ} C$ ?

22

1

20^{0}

C O_{2}

H e

3

Join BYJU'S Learning Program