If the reaction yield is 94.4%, what mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water? Mg (s) + 2H₂O (l) → Mg(OH)₂ (s) + H₂ (g) A)0.0962 B)0.0162 C)0.0485 D)0.219 E)0.204

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The balanced chemical equation is:Mg (s) + 2H₂O (l) → Mg(OH)₂ (s) + H₂ (g)1 mol Mg reacts with 2 mol H₂O to produce 1 mol H₂.The molar mass of Mg is 24.31 g/mol, and the molar mass of H₂ is 2.02 g/mol.Therefore, 4.73 g of Mg reacts with 1.83 g of H₂O to produce 0.0962 g of H₂.The reaction yield is 94.4%, so the actual mass of H₂ produced is 0.0962 g * 0.944 = 0.0910 g.Therefore, the correct answer is A) 0.0962.

If the Reaction Yield Is 94