Question

A 10 l flask contains 0.2 moles of ch4 and 0.3 mole of hydrogen at 25°c and which makes non reacting gaseous mixture then the total pressure inside the flask is

Answer 1

Answer:- 1.223 atm

Solution:- Moles of methane = 0.2

moles of hydrogen = 0.3

Volume = 10 L

Temperature = 25 + 273 = 298 K

Using ideal gas equation we could calculate the partial pressure of each gas.

PV = nRT

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

Partial pressure of methane = $\frac{0.2*0.0821*298}{10}$

Partial pressure of methane = 0.489 atm

Similarly, partial pressure of hydrogen = $\frac{0.3*0.0821*298}{10}$

partial pressure of hydrogen = 0.734 atm

As per Dalton's law of partial pressure, "Total pressure of a gaseous mixture is the sum of partial pressures of the gaseous species present in it."

So, total pressure of the gaseous mixture = 0.489 atm + 0.734 atm  = 1.223  atm

Hence, the total pressure of the mixture is 1.223 atm.