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If 8.40 moles of sulfur dioxide are produced when this reaction occurs, how many moles of oxygen were required?

User Nypan
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1 Answer

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Final answer:

12.6 moles of oxygen were required to produce 8.40 moles of sulfur dioxide based on the stoichiometry of the chemical equation 2H₂S (g) + 3O₂ (g) → 2SO₂ (g) + 2H₂O(g).

Step-by-step explanation:

To determine how many moles of oxygen were required to produce 8.40 moles of sulfur dioxide, we must use the chemical reaction provided and apply stoichiometry principles:

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

According to the reaction, it takes 3 moles of oxygen (O₂) to produce 2 moles of sulfur dioxide (SO₂). To find out the amount of oxygen needed for 8.40 moles of SO₂, we set up a proportion based on the coefficients in the balanced equation:

(3 moles O₂ / 2 moles SO₂) = x moles O₂ / 8.40 moles SO₂

Solving for x, we find that:

x = (3/2) * 8.40 moles SO₂

x = 12.6 moles O₂

Therefore, 12.6 moles of oxygen were required to produce 8.40 moles of sulfur dioxide.

User Dexygen
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