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AP Chem help needed

Post by JaySav »

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?
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Re: AP Chem help needed

Post by ChenBeier »

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
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