Question

Carbon monoxide and molecular oxygen react to form carbon dioxide. A 50.0 L reactor at 25.0 oC is charged with 1.00 bar of CO. The gas is then pressurized with O2 to give a total pressure of 3.52 bar. The reactor is sealed, heated to 350 oC to drive the reaction to completion, and cooled back to 25.0 oC. Compute the final partial pressure of each gas (in bar).

Answer 1

Answer:

CO = zero

CO2 =1 bar

O2  = 2.02 bar

Explanation:

We are given

initial pressure of CO = 1bar

total pressure = 3.52 bar

so initial pressure of O2 = 3.52 - 1 = 2.52 bar

the reaction is

2CO + O2 →  2CO2

using the unitary method

2 moles of CO2 → 1 mole of O2

1  bar of CO → $\frac{1}{2} * 1= 0.5 bar$ (required)

but we have more oxygen present , that means CO is the limiting reagent

• Final pressure of CO will be zero as it is the limiting reagent so it will be consumed completely
• 1 bar of CO → $\frac{2mol CO2}{2mol CO} * 1= 1 bar$ of CO2
• 2.52 bar O2 (initially) - 0.5 bar (reacted) = 2.02bar O2