Final answer:
The actual yield of calcium chloride formed from the reaction of 95 grams of calcium carbonate with hydrochloric acid, with a percent yield of 82.15%, is 86.5 grams.
option d is the correct
Step-by-step explanation:
The question involves a stoichiometry calculation to find the actual amount of calcium chloride formed when calcium carbonate reacts with hydrochloric acid, given the percent yield of the reaction. We start with 95 grams of calcium carbonate and are told the percent yield is 82.15%. To find the actual yield of calcium chloride, we must first calculate the theoretical yield and then apply the percent yield.
Firstly, we must write the balanced chemical equation for the reaction:
CaCO₃ + 2 HCl → CaCl₂ + CO₂ + H₂O
From the molar masses, 100 grams of CaCO₃ (the approximate molar mass of calcium carbonate) would theoretically yield 111 grams of CaCl₂ (the molar mass of calcium chloride). Therefore, 95 grams of CaCO₃ would theoretically yield:
(95 g CaCO₃) x (111 g CaCl₂ / 100 g CaCO₃) = 105.45 g of CaCl₂ (theoretical yield)
Then, we apply the percent yield:
(105.45 g) x (82.15% / 100) = 86.5 grams of CaCl₂ (actual yield)
Therefore, the correct answer is D. 86.5 grams of calcium chloride were actually formed.