If 22.4 liters of H2(g) is mixed with 11.2 liters of Cl2(g), both at STP, how many moles of HCl(g) will be formed after the reaction is complete?

Model Answer & Options

Source: Extra Practice

1.0 mole

2.0 moles

0.5 mole

1.5 moles

Explanation

The balanced chemical equation is H2(g) + Cl2(g) → 2HCl(g). At STP, 1 mole of any gas occupies 22.4 L. Here, moles of H2 = 22.4/22.4 = 1.0 mol, and moles of Cl2 = 11.2/22.4 = 0.5 mol. According to the stoichiometry, 1 mole of H2 requires 1 mole of Cl2. Since we only have 0.5 mol of Cl2, Cl2 is the limiting reagent. The amount of product is determined by the limiting reagent: 1 mole of Cl2 produces 2 moles of HCl, so 0.5 mole of Cl2 will produce (0.5 × 2) = 1.0 mole of HCl.

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