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)0.102 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)From the equation, we can see that 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, 4.73 g of Mg is equal to 4.73 g / 24.31 g/mol = 0.194 mol of Mg.And 1.83 g of H₂O is equal to 1.83 g / 18.02 g/mol = 0.102 mol of H₂O.Since Mg is the limiting reactant, we will use the moles of Mg to calculate the moles of H₂ produced.According to the balanced chemical equation, 1 mole of Mg produces 1 mole of H₂.Therefore, 0.194 mol of Mg will produce 0.194 mol of H₂.Finally, we can convert the moles of H₂ to grams using the molar mass of H₂:0.194 mol of H₂ * 2.02 g/mol = 0.392 g of H₂Therefore, the mass of hydrogen produced by the reaction is 0.392 g.

What Mass in Grams of Hydrogen Is Produced by the Reaction