How many grams of H₂ gas gas can be produced by the reaction of 27.0 grams of Al(s) with an excess of dilute hydrochloric acid in the reaction shown below?
2 Al(s) + 6 HCl(aq) → 2 AlCl₃(aq) + 3 H₂(g)

Question

Quizplus · Accepted Answer

To determine the grams of gas produced, we need to calculate the moles of gas produced using stoichiometry.

First, calculate the moles of Al(s) using its molar mass of 26.98 g/mol:
27.0 g Al × (1 mol Al/26.98 g Al) = 1.00 mol Al

Since the reaction ratio between Al(s) and H2(g) is 2:3, we can use the mole of Al(s) to calculate the moles of H2(g):
1.00 mol Al × (3 mol H2/2 mol Al) = 1.50 mol H2

Now that we have the moles of H2(g), we can use its molar mass of 2.02 g/mol to calculate the grams of H2(g) produced:
1.50 mol H2 × (2.02 g H2/1 mol H2) = 3.03 g H2

Therefore, the answer is (C) 3.03 g.

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