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

Using the balanced chemical equation for the combustion of hydrogen sulfide, we find that 7.05 moles of oxygen gas are needed to completely burn 4.7 moles of hydrogen sulfide.

Step-by-step explanation:

The chemical reaction between hydrogen sulfide (H2S) and oxygen (O2) to produce sulfur dioxide (SO2) and water (H2O) can be represented by the balanced equation: 2 H2S (g) + 3 O2 (g) → 2 SO2 (g) + 2 H2O(g).

To determine the number of moles of oxygen gas required to completely burn 4.7 moles of hydrogen sulfide, we can use stoichiometry based on the balanced equation.

From the equation, every 2 moles of H2S require 3 moles of O2. Hence, for 4.7 moles of H2S:

(4.7 moles H2S) * (3 moles O2 / 2 moles H2S) = 7.05 moles O2

Therefore, 7.05 moles of oxygen gas would be needed to completely burn 4.7 moles of hydrogen sulfide.