Final answer:
To produce 4.35 mol of water, approximately 161.24 g of calcium hydroxide is needed.
Step-by-step explanation:
To determine the mass of calcium hydroxide needed to produce 4.35 mol of water, we need to use the balanced chemical equation and the stoichiometry of the reaction. From the balanced equation, we can see that for every 2 moles of water produced, 1 mole of calcium hydroxide is needed. Therefore, we can set up a proportion:
1 mol Ca(OH)₂ / 2 mol H₂O = x mol Ca(OH)₂ / 4.35 mol H₂O
Solving for x, we find that x = (1 mol Ca(OH)₂ / 2 mol H₂O) * 4.35 mol H₂O = 2.175 mol Ca(OH)₂
To convert moles to grams, we need to use the molar mass of calcium hydroxide, which is approximately 74.1 g/mol. Therefore, the mass of calcium hydroxide needed is 2.175 mol * 74.1 g/mol = 161.24 g.