What is the mass of H2 and O2 produced water electrolysis?

[HelloCthulhu]

Homework Statement

2 moles of H2O undergoes electrolysis at 15 amps for 1 hour. What is the mass of H2 and O2 gas produced?

Homework Equations

4 H+(aq) + 4e−→ 2H2(g)

2 H2O(l) → O2(g) + 4 H+(aq) + 4e−

Faraday's Law of Electrolysis
Q = n(e-) x F

The Attempt at a Solution

F = 96500C

(15*3600s*4g)/(F*4)=0.55g H2

(15*3600s*32g)/(F*4)=4.47g O2

 

[PhyStudent20]

Isn't that the correct solution?

 

[HelloCthulhu]

Isn't that the correct solution?

I think so. I've seen a few other methods, but this one seems the simplest.

 

[James Pelezo]

You can check your calculation accuracy by converting the gram - values to moles. For water, moles H₂(g) produced should be 2x moles of O₂ produced. Your numbers do confirm this => 0.55g H₂ = 0.28 mole H₂ and 4.47g O₂ = 0.14 mole O₂ which is 2:1 ratio of H to O. Good job.