Given the following equations:

Question

2 H2O2 (aq) → 2 H2O (l) + O2 (g) and
C2H4 (g) + 3 O2 (g) → 2 CO2 (g) + 2 H2O (l)
The first reaction is the decomposition of hydrogen peroxide into water and oxygen gas. The oxygen gas generated in the first reaction is used in the second (combustion) reaction.
If I have 7.6 g of H2O2, how many grams of CO2 can I produce from the set of reactions?

Answer 1

each two moles of hydrogen peroxide produces one mole of oxygen gas

each three moles of oxygen gas produces two moles of carbon dioxide gas

so the moles of carbon dioxide is one third the starting moles of hydrogen peroxide

use the molar masses to find the amount produced

Answer 2

50.0 g of water are decomposed. 25.5L of Oxygen gas are produced as a result. What is the percent yield according to the following reaction. H2O --> H2 + O2 *