Question

Study the balanced chemical reaction.

H2 + O2 → H2O2
(M H2 = 2.02 g/mol; M H2O2​ = 34.02 g/mol)

If 100.0 g of hydrogen peroxide (H2O2) is produced, what percent of the product is hydrogen?

A) 50.0% is hydrogen.
B) 94.1% is hydrogen.
C) 5.94% is hydrogen.
D) 12.5% is hydrogen.

Answer 1

C) 5.94% is hydrogen.

Step-by-step explanation:

H2 H2O2

2.02 g/mol; 34.02 g/mol

x :: 100.0

x=100×2.02/34.02=5.94%

Answer 2

Option C. 5.94% is hydrogen.

Step-by-step explanation:

From the question given, we obtained the following:

Molar Mass of H2O2 = 34.02 g/mol

Molar Mass of H2 = 2.02 g/mol

Mass of H2O2 produced = 100g

H2 + O2 → H2O2

From the equation,

2.02g of Hydrogen produced 34.02g of H2O2.

Therefore, Xg of H2 will produce 100g of H2O2 i.e

Xg of H2 = (2.02x100)/34.02 = 5.94g

Now, we can calculate the percentage of H2 in H2O2 produced by doing the following:

% Mass of H2 in H2O2 = (5.94/100) x 100 = 5.94%