Answer:
Partial pressure of of CO₂ in the product mixture is 0,20atm
Explanation:
The balance equation is:
2CO(g) + O₂(g) → 2CO₂(g)
Total pressure of CO(g) and O₂(g) gases before reaction at 100,0°C and 1,0L is 1,50 atm. You can say:
X₁ + Y₁ = 1,50atm <em>(1)</em>
Where X₁ is initial partial pressure CO and Y₁ is initial partial pressure of O₂
After reaction partial pressures are:
X₂ = X₁ - 2n = 0; <em>2n = X₁</em>
Y₂ = Y₁ - n
Z₂ = 2n
Where Z₂ is final partial pressure of CO₂
After reaction pressure at 100,0°C and 1,0L is 1,40 atm, that means:
1,40 atm = (Y₂ + Z₂)
1,40 atm = Y₁ - n + 2n
1,40atm = Y₁ + n
1,40 atm = Y₁ + X₁/2 <em>(2)</em>
Replacing (1) in (2)
1,40 atm = 1,50atm - X₁ + X₁/2
-0,10 atm = - X₁/2
<em>0,20 atm = X₁</em>.
As 2n = X₁; 2n =<em> Z₂ = 0,20 atm</em>
I hope it helps!
