When firing zinc sulfide, 0.5 mol of zinc oxide was obtained. How much sulfur (IV) oxide was formed as a result of this process?

Reaction equation:
2ZnS + 3O2 = to => 2ZnO + 2SO2
From the conditions of the job:
n (ZnO) = 0.5 mol,
Both zinc oxide and sulfur oxide have the same coefficient in the equation. Therefore, the number of moles of these substances are equal:
n (SO2) = n (ZnO) = 0.5 mol
Hence:
B (SO2) = Vm ⋅ n (SO2) = 22.4 ⋅ 0.5 = 11.2 L

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