Question

Hydrogen sulfide gas, which smells like rotten eggs, burns in air to produce sulfur dioxide and water. How many moles of oxygen gas would be needed to completely burn 4.7 moles of hydrogen sulfide? __H₂S(g) + __O₂ (g) => __SO₂(g) + __H₂O(g)

Answer 1

To burn 4.7 moles of hydrogen sulfide completely, 7.05 moles of oxygen gas are needed, as per the balanced chemical equation for the combustion of hydrogen sulfide.

Step-by-step explanation:

To determine the number of moles of oxygen gas needed to completely burn 4.7 moles of hydrogen sulfide, we look at the balanced chemical equation for the reaction:

2H₂S (g) + 3O₂ (g) → 2SO₂ (g) + 2H₂O(g)

This balanced equation indicates that 2 moles of H₂S react with 3 moles of O₂. To find out how much O₂ is needed for the combustion of 4.7 moles of H₂S, we set up a proportion:

× moles O₂ = (4.7 moles H₂S) × (3 moles O₂ / 2 moles H₂S)

After performing the calculation, × moles O₂ = 7.05 moles O₂. Therefore, 7.05 moles of oxygen are required to completely react with 4.7 moles of hydrogen sulfide.