If the reaction yield is 88.2%,what mass in grams of hydrogen is produced by the reaction of 7.73 g of magnesium with 1.31 g of water?
Mg (s) + 2H₂O (l) → Mg(OH) ₂(s) + H₂(g)

Question

Quizplus · Accepted Answer

The balanced chemical equation is:Mg (s)+ 2H₂O (l)→ Mg(OH)₂(s)+ H₂(g)1 mole of Mg reacts with 2 moles of H₂O to produce 1 mole of H₂.The molar mass of Mg is 24.31 g/mol, and the molar mass of H₂ is 2.02 g/mol.Therefore, 7.73 g of Mg will react with 1.31 g of H₂O to produce 0.0646 g of H₂.The reaction yield is 88.2%, so the actual mass of H₂ produced will be 0.0646 g * 0.882 = 0.0568 g.

If the Reaction Yield Is 88