The percentage yield of a reaction is 24.3%. If an experimental value of 114.86 g of product is obtained, what would be the theoretical value?

Question

BlackTom AI · Accepted Answer

We start by identifying the relationship between actual yield, theoretical yield, and percent yield. Percent yield is defined as (actual yield / theoretical yield) × 100.

Option-by-option analysis:
- 27.87 g: If this were the theoretical yield, then the percent yield would be (114.86 / 27.87) × 100 ≈ 412.5%, which is impossible for a typical reaction. This option is clearly inconsistent with the definition of percent yield.
- 86.99 g: If this were the theoretical yield, the percent yield would be (114.86 / 86.99) × 100 ≈ 132.1%, still impossible since percent yield cannot exceed 100% in ordinary reactions. This option is not viable.
- 424.67 g: If this were the theoretical yield, the percent yield would be (114.86 / 424.67) × 100 ≈ 27.1%. This is a plausible value for percent yield, though it does not match the given 24.3% exactly. It would imply a yield close to 27%, which could occur if there were rounding or measurement issues.
- 357.81 g: If this were the theoretical yield, the percent yield would be (114.86 / 357.81) × 100 ≈ 32.1%, which is again a plausible percentage but not matching the stated 24.3% yield.
- 92.41 g: If this were the theoretical yield, the percent yield would be (114.86 / 92.41) × 100 ≈ 124.5%, which is not physically meaningful for a standard reaction; percent yield cannot exceed 100% under ordinary conditions.

Now, focusing on the key formula: actual = (percent yield) × (theoretical yield) / 100. Rearranging gives theoretical yield = actual × 100 / percent yield. Using actual = 114.86 g and percent yield = 24.3%, we calculate theoretical yield ≈ 114.86 × 100 / 24.3 ≈ 114.86 × 4.115226 = approximately 473 g.

Compare this to the provided options: none of the listed options equals roughly 473 g. The closest option is 424.67 g, which would correspond to a percent yield of about 27.1% if used with the same formula. This suggests a possible inconsistency between the stated percent yield (24.3%) and the answer choices, or a rounding/recording discrepancy in the problem.

In summary, applying the standard definition yields a theoretical value near 473 g, but none of the answer choices matches that result exactly. The option 424.67 g would imply a different percent yield (around 27%), not 24.3%, indicating a mismatch between the provided percent yield and the option set.

The percentage yield of a reaction is 24.3%. If an experimental value of 114.86 g of product is obtained, what would be the theoretical value?

View Explanation

Log in for full answers

Similar Questions

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?

2.10 Determine percentage yields for reactions

If the reaction in question Q16 produces 24.6 g of sulfur trioxide, what is the % yield of the reaction

Consider the following equation 2 Mg (s) + O2 (g) → 2 MgO (s) When 40.0 g of O2 completely react with Mg, the actual yield of MgO is 83.6 g. What is the percent yield? Given molar mass of MgO is 40.31 g/mol.

The formula to calculate the yield percentage is

The formula to calculate the yield percentage is

Sn3(PO4)4 + 6 Na2CO3 → 3 Sn(CO3)2 + 4 Na3PO4 36 grams of tin (IV) phosphate Sn3(PO4)4 is mixed with an excess of sodium carbonate Na2CO3. In the lab 29.8 grams of tin (IV) carbonate Sn(CO3)2 are actually formed. What is the percent yield?

More Practical Tools for Students Powered by AI Study Helper

Homework AI Solver

Stylized AI Paper Writer

Plagiarism Checker Assistant

Citation AI Academic Writing Tool

In-Class Translation Assistant

AI Note Generator

AI Quiz Answers

Past Exam Questions from University Test Bank

Smart Practice Assistant

Adaptive Practice

Making Your Study Simpler