3. Calcium carbonate can react with sulfuric acid to produce Calcium sulfate, water, and Carbon dioxide. 54.1 g CaCO3 and 42.4 g H2S04 react together and produce 59.2 g Calcium Sulfate. CaCO3(s) + H2SO4(ag) → CasO4 (ag) + H2O(1) + CO2 (g) ww
3. Calcium carbonate can react with sulfuric acid to produce Calcium sulfate, water, and Carbon dioxide. 54.1 g CaCO3 and 42.4 g H2S04 react together and produce 59.2 g Calcium Sulfate. CaCO3(s) + H2SO4(ag) → CasO4 (ag) + H2O(1) + CO2 (g) ww
Introductory Chemistry: An Active Learning Approach
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Chapter10: Quantity Relationships In Chemical Reactions
Section: Chapter Questions
Problem 70E: Classify each of the following statements as true or false: a Coefficients in a chemical equation...
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Can you please help me with question 3.
![**Percent Yield:**
**Percent yield** is a measure of the efficiency of a chemical reaction and is defined as the ratio of the actual yield to the theoretical yield, expressed as a percentage.
The *theoretical yield* of an experiment is the amount of product calculated from a stoichiometry problem after identifying the limiting reactant. However, when doing an experiment there are many opportunities for error such that the *actual yield*, the amount obtained in the lab after the chemical reaction occurred, is different from the theoretical yield. The difference in the actual and theoretical yield can be written as a percent ratio, *percent yield*.
\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100 \]
Where:
- **Actual Yield** is the quantity of product actually obtained from a reaction.
- **Theoretical Yield** is the quantity of product expected based on stoichiometric calculations.
### For the following problems, identify the limiting reactant and calculate the percent yield.
1. **In an experiment, the actual yield was 3.26 grams and the theoretical yield was 3.42 grams. What was the percent yield?**
\[ \text{Percent Yield} = \left( \frac{3.26 \, \text{g}}{3.42 \, \text{g}} \right) \times 100 = 95.32\% \]
2. **A reaction between 2.1 L of Carbon dioxide and 6.7 g of Calcium hydroxide produces Calcium Carbonate and water. However, when the experiment was done in the lab, scientists only measured a production of 9.11 grams of Calcium Carbonate.**
\[ \text{CO}_2 (\text{g}) + \text{Ca}(\text{OH})_2 (\text{aq}) \rightarrow \text{CaCO}_3 (\text{s}) + \text{H}_2\text{O} (\text{l}) \]
3. **Calcium carbonate can react with sulfuric acid to produce Calcium sulfate, water, and Carbon dioxide. 54.1 g CaCO₃ and 42.4 g H₂SO₄ react together and produce 59.2 g Calcium Sulfate.**
\[ \text{CaCO}_3 (\text{s}) +](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F78637c7f-7c6b-4f2a-8230-52099e22ee3b%2Ff643af83-c239-4ca6-be52-89f5059cf4e3%2F2mv9of_processed.png&w=3840&q=75)
Transcribed Image Text:**Percent Yield:**
**Percent yield** is a measure of the efficiency of a chemical reaction and is defined as the ratio of the actual yield to the theoretical yield, expressed as a percentage.
The *theoretical yield* of an experiment is the amount of product calculated from a stoichiometry problem after identifying the limiting reactant. However, when doing an experiment there are many opportunities for error such that the *actual yield*, the amount obtained in the lab after the chemical reaction occurred, is different from the theoretical yield. The difference in the actual and theoretical yield can be written as a percent ratio, *percent yield*.
\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100 \]
Where:
- **Actual Yield** is the quantity of product actually obtained from a reaction.
- **Theoretical Yield** is the quantity of product expected based on stoichiometric calculations.
### For the following problems, identify the limiting reactant and calculate the percent yield.
1. **In an experiment, the actual yield was 3.26 grams and the theoretical yield was 3.42 grams. What was the percent yield?**
\[ \text{Percent Yield} = \left( \frac{3.26 \, \text{g}}{3.42 \, \text{g}} \right) \times 100 = 95.32\% \]
2. **A reaction between 2.1 L of Carbon dioxide and 6.7 g of Calcium hydroxide produces Calcium Carbonate and water. However, when the experiment was done in the lab, scientists only measured a production of 9.11 grams of Calcium Carbonate.**
\[ \text{CO}_2 (\text{g}) + \text{Ca}(\text{OH})_2 (\text{aq}) \rightarrow \text{CaCO}_3 (\text{s}) + \text{H}_2\text{O} (\text{l}) \]
3. **Calcium carbonate can react with sulfuric acid to produce Calcium sulfate, water, and Carbon dioxide. 54.1 g CaCO₃ and 42.4 g H₂SO₄ react together and produce 59.2 g Calcium Sulfate.**
\[ \text{CaCO}_3 (\text{s}) +
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