According to the following reaction, how many moles of oxygen gas are necessary to form 0.543 moles water?
hydrogen sulfide (g) + oxygen (g) water (l) + sulfur dioxide (g)
2H2S+ 3O2 >> 2H2O+ 2SO2
so you need 3/2 moles*.543
To determine the number of moles of oxygen gas (O₂) necessary to form 0.543 moles of water (H₂O), we need to examine the balanced equation for the reaction mentioned.
The balanced equation for the reaction is:
2 H₂S (g) + 3 O₂ (g) → 2 H₂O (l) + 2 SO₂ (g)
From the balanced equation, we can see that for every 3 moles of oxygen gas (O₂), we obtain 2 moles of water (H₂O).
To find the number of moles of oxygen gas required to produce 0.543 moles of water, we can set up a proportion:
(3 mol O₂) / (2 mol H₂O) = (x mol) / (0.543 mol H₂O)
Cross-multiplying and solving for x, we find:
x = (3 mol O₂ * 0.543 mol H₂O) / (2 mol H₂O)
x ≈ 0.817 mol O₂
Therefore, approximately 0.817 moles of oxygen gas are necessary to form 0.543 moles of water.