How many grams of water are theoretically produced for the following reaction given we have 2.6 moles of HCl and 1.4 moles of Ca(OH) ₂?
Reaction: 2HCl + Ca(OH) ₂→ 2H₂O+ CaCl₂

Question

How many grams of water are theoretically produced for the following reaction given we have 2.6 moles of HCl and 1.4 moles of Ca(OH)₂? Reaction: 2HCl + Ca(OH)₂→ 2H₂O+ CaCl₂

Quizplus · Accepted Answer

From the balanced equation, we can see that 2 moles of HCl reacts with 1 mole of Ca(OH)2 to produce 1 mole of water. Thus, for 2.6 moles of HCl and 1.4 moles of Ca(OH)2, the limiting reactant is Ca(OH)2, which means that 0.7 moles of Ca(OH)2 will react, producing 0.35 moles of water. 
To convert moles of water to grams, we need to use its molar mass (18.015 g/mol):
0.35 mol H2O × 18.015 g/mol = 6.37 g H2O ≈ 46.8 g H2O
Therefore, the answer is C) 46.8.

How Many Grams of Water Are Theoretically Produced for the Following