Question

A 10 L flask contains 0.2 mole of ${CH}_4$ and 0.3 mole of hydrogen at ${25}^{0}C$ and which makes non-reacting gaseous mixture. Then the total pressure inside the flask is:

• A. 1.22 atm
• B. 0.5 atm
• C. 0.61 atm
• D. 2.20 atm

Answer 1

The correct option is A 1.22 atm

Moles of methane = 0.2

Moles of hydrogen = 0.3

Volume = 10 L

Temperature = 25 + 273 = 298 K

PV = nRT

P = $\frac{nRT}{V}$

Partial pressure of methane = $\frac{0.2\times 0.0821\times 208}{10}$

Partial pressure of methane = 0.489 atm

Partial pressure of hydrogen = $\frac{0.3\times 0.0821\times 208}{10}$

Partial pressure of methane = 0.734 atm

Total Pressure of the gaseous mixture = 0.489 atm + 0.734 atm =1.22 atm