HELP CHEMISTRY ASAP

Question

Given the following equation:

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

7.6 g H₂O₂ x 1 mole H₂O₂/34 g = 0.2235 moles H₂O₂

moles O₂ produced = 0.2235 moles H₂O₂ x 1 mole O₂/2 moles H₂O₂ = 0.1118 moles O₂

0.1118 moles O₂ x 2 moles CO₂/3 moles O₂ x 44 g/mole CO₂ = 3.3 g CO₂ produced (2 sig. figs.)

(NOTE: this assumes that C₂H₄ is NOT limiting in reaction #2)

Answer 2

Did you calculate the molecular weights in the first reaction, and then find the # of moles of O2 produced?