Calcium oxide reacts with excess carbon dioxide to produce calcium carbonate. Junior Chemist isolates 5.9 g of calcium carbonate at the end of her experiment. Earlier she had calculated (from stoichiometry) a yield of 12.8 g. What is her % yield?

Question

Calcium oxide reacts with excess carbon dioxide to produce calcium carbonate.  Junior Chemist isolates 5.9 g of calcium carbonate at the end of her experiment.  Earlier she had calculated (from stoichiometry) a yield of 12.8 g.  What is her % yield?

BlackTom AI · Accepted Answer

We need to evaluate the percent yield using the formula: percent yield = (actual yield / theoretical yield) × 100.
Option 1: 46% — Compare 5.9 g (actual) to 12.8 g (theoretical). (5.9 / 12.8) × 100 ≈ 0.4609 × 100 ≈ 46.1%. This matches the calculated value, so this option is consistent with the data.
Option 2: 59% — This would imply (actual / theoretical) ≈ 0.59. If you reverse it, 12.8 × 0.59 ≈ 7.55 g, which does not equal the actual 5.9 g. The ratio is too high to be supported by the given numbers.
Option 3: 78% — This would require actual ≈ 0.78 × 12.8 ≈ 9.984 g. Since the reported actual yield is 5.9 g, this percentage would overestimate yield by a wide margin.
Option 4: 128% — A yield over 100% would imply the actual mass exceeded the theoretical maximum, which is not physically possible under normal stoichiometric conditions for a single reaction, so this is not reasonable here.
Option 5: 217% — Similar to 128%, this exceeds 100% by a large margin and contradicts the concept of yield being a fraction of the theoretical amount, making it an incoherent choice for this scenario.
In this context, the correct interpretation of the data yields a percent that closely matches 46%, accurately reflecting the ratio of actual to theoretical yield. The other options either misapply the ratio, rely on arithmetic that would produce implausible results, or misinterpret what percent yield represents.

Calcium oxide reacts with excess carbon dioxide to produce calcium carbonate. Junior Chemist isolates 5.9 g of calcium carbonate at the end of her experiment. Earlier she had calculated (from stoichiometry) a yield of 12.8 g. What is her % yield?

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