Given the reaction 2SO2(g) + O2(g) → 2SO3(g), if 8.0 mol of SO2 and 4.0 mol of O2 are reacted, what is the theoretical yield of SO3 (in moles)?

• A. 4.0 mol
• B. 8.0 mol
• C. 2.0 mol
• D. 6.0 mol

Answer: (A)

Verified step by step guidance

1. Write down the balanced chemical equation: \$2SO_2(g) + O_2(g) \rightarrow 2SO_3(g)$.
2. Identify the initial moles of reactants: 8.0 mol of \(SO_2\) and 4.0 mol of \(O_2\).
3. Determine the mole ratio from the balanced equation: 2 mol \(SO_2\) reacts with 1 mol \(O_2\) to produce 2 mol \(SO_3\).
4. Find the limiting reactant by comparing the mole ratio of the given amounts: calculate how much \(O_2\) is needed for 8.0 mol \(SO_2\) and how much \(SO_2\) is needed for 4.0 mol \(O_2\).
5. Use the limiting reactant to calculate the theoretical yield of \(SO_3\) using the mole ratio from the balanced equation.