How many grams of H2O2(l) would have to react to produce 28.9 kJ of energy?

Question

The following thermochemical equation is for the reaction of hydrogen peroxide(l) to form water(l) and oxygen(g).

1. 2H₂O₂(l)2H₂O(l) + O₂(g)    H = -196 kJ

How many grams of H₂O₂(l) would have to react to produce 28.9 kJ of energy?

Answer 1

It looks like 2 mol H₂O₂ releases 196 Joules of energy once it reacts. Based on this ratio, 1 mol H₂O₂ should release 98 Joules of energy once it reacts.

If you want to create 28.9 kJ or 28900 Joules, you need 294.898 mol H₂O₂ (28900/98).

The molar mass of H₂O₂ is 1.01 + 1.01 + 16.00 + 16.00 = 34.02 g/mol.

Multiply 294.898 mol H₂O₂ x 34.02 g/mol and you should get 10,030 g H₂O₂ or 10.03 kg H₂O₂

Answer 2

Hi Alexandria! Here's a very detailed break-down of your problem. It's my first video, so please let me know if there's anything I could adjust and I am happy to answer any follow-up questions that you have. :)

Gigi