Chemistry Homework

Question

According to the following reaction, how many moles of water will be formed upon the complete reaction of 0.640 moles hydrogen sulfide with excess oxygen gas?

hydrogen sulfide (g) + oxygen (g) water (l) + sulfur dioxide (g)

Answer 1

Let's turn the word equation into a chemical equation and balance it.

hydrogen sulfide (g) = H₂S(g)

oxygen (g) = O₂(g)

water (l) = H₂O(l)

sulfur dioxide = SO₂(g)

2H₂S(g) + 3O₂(g) ==> 2H₂O(l) + 2SO₂(g) ... balanced equation

From the balanced equation we see that TWO moles of H₂O are formed from TWO moles of H₂S (when O₂ is in excess and not limiting the production of water). So, the mole ratio of H₂O to H₂S is 1 : 1.

0.640 mols H₂S x 1 mol H₂O / 1 mol H₂S = 0.640 mols H₂O formed