First slide

Kinetic theory of ideal gases

Question

A vessel contains 0.5 g of hydrogen and 0.8 g of oxygen. The volume of vessel is $\frac{5}{28} m^{3}$ while its temperature is maintained at 300 K. Then the pressure of the mixture is $(M_{H_{2}} = 2, M_{O_{2}} = 32, R = \frac{25}{3} J - m o l^{- 1} K^{- 1})$ .

Moderate

A

$385 N m^{- 2}$
B

$38.5 N m^{- 2}$
C

$3850 N m^{- 2}$
D

$3.85 N m^{- 2}$

Solution

By Dalton’s law,
$\begin{array}{l} P = P_{H_{2}} + P_{O_{2}} \\ = \frac{n_{H_{2}} R T}{V} + \frac{n_{O_{2}} R T}{V} = (\frac{0.5}{2} + \frac{0.8}{32}) (\frac{25}{3}) (\frac{300}{(\frac{5}{28})}) = 3850 {Nm}^{- 2} \end{array}$

Get Instant Solutions

When in doubt download our app. Now available Google Play Store- Doubts App

Recieve an sms with download link

Doubts App

OR

SCAN ME

Doubts App

Doubts App