Chemistry Forum

Hydrogen peroxide is oxidized with permanganate solution to produce oxygen gas by the following reaction:

2H + H₂O₂ + 2MnO₄ -> 2MnO₂ + 4H₂O + 3O₂

In the lab a student mixed 30.0 mL of 0.30 M hydrogen peroxide solution with 30.0 mL of 0.30 M potassium permanganate solution. The oxygen that was produced was collected by water displacement at 298 K and 1.00 atm of pressure. The volume of oxygen collected was 178 mL. (Ignore the effect of water vapor in the collection tube here.)

a.) What is the limiting reactant?

b.) What is the theoretical yield of oxygen gas, in milliliters?

c.) What is the percent yield of oxygen gas?

a. The given equation is not balanced. Also charges are missing. Tipp: in neutral solution Oxidation is done by Adding of OH- and gaining H₂O .The reduction is vise versa.
If you have the right equation read how many mol H₂O₂ correspond to Permanganat. Your mixture is equimolar!

b. Use molar volume or ideal gas law.

c. Yield = practical volume/theoretical volume