For the reaction, calculate how many moles of the product form when 2.05 mol of O2 completely reacts.

Assume that there is more than enough of the other reactant.

2H2 (g) + O2 (g) →2H2O (l)

Question

Chemistry

Jordyn Krueger

18 August, 09:52

For the reaction, calculate how many moles of the product form when 2.05 mol of O2 completely reacts.

Assume that there is more than enough of the other reactant.

2H2 (g) + O2 (g) →2H2O (l)

+3

Answers (1)

Know the Answer?

Chad Lyons · Answer 1

n H2O (l) = 4.1 mol

Explanation:

2H2 (g) + O2 (g) → 2H2O (l)

∴ n O2 (g) = 2.05 mol

⇒ n H2O (l) = (2.05 mol O2) * (2 mol H2O / mol O2)

⇒ n H2O (l) = 4.1 mol

For the reaction, calculate how many moles of the product form when 2.05 mol of O2 completely reacts.Assume that there is more than enough of the other reactant.2H2 (g) + O2 (g) →2H2O (l)

For the reaction, calculate how many moles of the product form when 2.05 mol of O2 completely reacts.

Assume that there is more than enough of the other reactant.

2H2 (g) + O2 (g) →2H2O (l)