Question

. A 2L container at 300K holds a gaseous mixture of 0.2g of He, 1.6 g of CH, and 2.2 g of CO,. The
pressure of mixture is
1) 3.6 atm
2) 1.8 atm
3) 4.8 atm
4) 2.4 atm​

Answer 1

Answer:

no answer is 2.4 4) trust me it's not 1.8, it can't be

Answer 2

Answer:

The pressure for given gaseous mixture is 2.463 atm.

Explanation:

Given:  volume of container=2L, T =300K, R = 0.0821 Litreatmmol⁻¹K⁻¹

Moles of He $=\frac{0.2}{4} =0.05 moles$

Moles of CH₄ = $\frac{1.6}{16} =0.1 moles$

Moles of CO₂ =$\frac{2.2}{44} =0.05 moles$

Total moles in the mixture $n_{total}=0.05+0.1+0.05=0.2moles$

By ideal gas equation,

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

  ∴        $P=\frac{(0.2)(0.0821)(300)}{2} \\ \\ P=2.463atm$

Hence the pressure equals to 2.463 atm for gaseous mixture.