A 22.4 L high pressure reaction vessel is charged with 0.5930 mol of iron powder and 1.65 atm of oxygen gas at standard temperature.On heating,the iron and oxygen react according to the balanced reaction below. 4Fe(s) + 3O₂(g) → 2Fe₂O₃(s)
After the reaction vessel returns to standard temperature,and assuming the reaction goes to completion,what pressure of oxygen remains?

Question

Quizplus · Accepted Answer

According to the balanced chemical equation, 4 moles of Fe react with 3 moles of O2. Therefore, 0.5930 mol of Fe will react with (3/4) * 0.5930 = 0.4448 mol of O2. The initial pressure of O2 was 1.65 atm, and 0.4448 mol of O2 was consumed in the reaction. Therefore, the pressure of O2 remaining after the reaction is 1.65 atm - (0.4448 mol/1.65 atm) * 1 atm = 1.20 atm.

A 224 L High Pressure Reaction Vessel Is Charged with 0