Stoichiometry Practice Hydrogen sulfide gas reacts with oxygen gas to form sulfur dioxide and water according to the following equation. 2H_(2)S(g)+3O_(2)(g)arrow 2SO_(2)(g)+2H_(2)O(g) What volume of hydrogen sulfide is needed to react completely with 4.2 L oxygen? 4.2 L 8.4 L 1.9 L 2.8L

## Step 1The balanced chemical equation given is:### \(2H_{2}S(g) + 3O_{2}(g) \rightarrow 2SO_{2}(g) + 2H_{2}O(g)\)This equation tells us that 2 moles of hydrogen sulfide (H2S) react with 3 moles of oxygen (O2) to produce 2 moles of sulfur dioxide (SO2) and 2 moles of water (H2O).## Step 2The stoichiometry of the reaction is 2:3, which means that for every 3 moles of oxygen, 2 moles of hydrogen sulfide are required.## Step 3The problem provides that 4.2 L of oxygen is available. Since the stoichiometry of the reaction is 2:3, we can set up a proportion to find the volume of hydrogen sulfide needed.## Step 4The proportion is set up as follows:### ## Step 5Solving for x gives us the volume of hydrogen sulfide needed.