Question

Consider 1.56 grams of H2(g) produced by the following chemical reaction. 2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g) Determine if each of the following statements is True or False. The reaction requires 27.9 grams of H2O. [ Select ] The reaction also produces 1.55 grams of NaOH. [ Select ] The grams consumed will equal the grams produced in this chemical reaction.

Answer 1

The actual amount of substance each required or produced by the reaction is obtained by stoichiometry.

From the reaction equation;

2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)

Number of moles in  1.56 grams of H2(g) = 1.56 grams/2.00g/mol = 0.78 moles

If 2 moles of water yields 1 mole of H2

x moles of water yields 0.78 moles of H2

x = 2 × 0.78/1 = 1.56 moles of water

Mass of water required = 1.56 moles of water × 18 g/mol = 28 grams of water

The statement that the reaction requires 27.9 grams of H2O is true.

Also;

The number of moles in 1.55g of NaOH = 1.55g/40g/mol = 0.039 moles

If 2 moles of water produces 2 moles of NaOH

1.56 moles of water produces 1.56 × 2/2 = 1.56 moles of NaOH

Mass of NaOH = 1.56 moles of NaOH * 40 g/mol = 62.4 g of NaOH

The statement that the reaction also produces 1.55 grams of NaOH is false.

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