Question

Given the decomposition of hydrogen peroxide, calculate the moles of oxygen gas produced from 4.20 mol of H2O2.

2H2O2(l)→2H2O(l)+O2(g)

Answer 1

To calculate the moles of oxygen gas produced from 4.20 mol of H2O2, we need to use the stoichiometry of the reaction. For every 2 mol of H2O2, 1 mol of O2 is produced. So, 4.20 mol of H2O2 will produce 2.10 mol of O2.

Step-by-step explanation:

To calculate the moles of oxygen gas produced from 4.20 mol of H2O2, we can use the stoichiometry of the reaction. From the balanced equation: 2H2O2(l) → 2H2O(l) + O2(g), we can see that for every 2 mol of H2O2, 1 mol of O2 is produced.

So, for 4.20 mol of H2O2, we can set up a proportion:

(4.20 mol H2O2)/(2 mol H2O2) = (x mol O2)/(1 mol O2)

Solving for x, we find that x = 2.10 mol of O2.

Answer 2

2.10 moles of O₂

Step-by-step explanation:

2 H₂O₂ (l) → 2H₂O(l) + O₂(g)

In this reaction we say, that 2 moles of hydrogen peroxide can decompose to 2 moles of water and 1 mol of oyxgen.

So ratio is 2:1, according to stoichiometry.

If we apply a rule of three;

2 moles of hydrogen peroxide can decompose to 1 mol of oxygen

Then 4.20 moles of hydrogen peroxide may produced (4.20 . 1)/2 =

2.10 moles of O₂