2. A reaction between 2.1 L of Carbon dioxide and 6.7 g of Caleium 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. co2(g) + Ca(OH)2(aq) → CACO3(s) + H2O(1)
2. A reaction between 2.1 L of Carbon dioxide and 6.7 g of Caleium 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. co2(g) + Ca(OH)2(aq) → CACO3(s) + H2O(1)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Can you please help me with question 2.
![**Percent Yield:**
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**.
\[
\text{Percent Yield} = \left(\frac{\text{Actual Yield}}{\text{Theoretical Yield}}\right) \times 100\%
\]
---
**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?**
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.**
\[
\text{CO}_2(\text{g}) + \text{Ca(OH)}_2(\text{aq}) \rightarrow \text{CaCO}_3(\text{s}) + \text{H}_2\text{O}(\text{l})
\]
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.**
\[
\text{CaCO}_3(\text{s}) + \text{H}_2\text{SO}_4(\text{aq}) \rightarrow \text{CaSO}_4 (\text{aq}) + \text{H}_2\text{O} (\text{l}) + \text{CO}_2 (\text{g})
\]
4. **Carbon dioxide reacts with sodium hydroxide to form sodium carbonate and water. When 2.41 L of Carbon dioxide gas and 3.50 grams of Sodium hydroxide are reacted together in a lab, 4.75 grams of Sodium carbonate is produced.**
\[
\text{CO}_2(\text{g](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F78637c7f-7c6b-4f2a-8230-52099e22ee3b%2Fbc4eb116-8cd8-4b06-8195-09f6409dce09%2Fhulcuqb_processed.png&w=3840&q=75)
Transcribed Image Text:**Percent Yield:**
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**.
\[
\text{Percent Yield} = \left(\frac{\text{Actual Yield}}{\text{Theoretical Yield}}\right) \times 100\%
\]
---
**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?**
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.**
\[
\text{CO}_2(\text{g}) + \text{Ca(OH)}_2(\text{aq}) \rightarrow \text{CaCO}_3(\text{s}) + \text{H}_2\text{O}(\text{l})
\]
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.**
\[
\text{CaCO}_3(\text{s}) + \text{H}_2\text{SO}_4(\text{aq}) \rightarrow \text{CaSO}_4 (\text{aq}) + \text{H}_2\text{O} (\text{l}) + \text{CO}_2 (\text{g})
\]
4. **Carbon dioxide reacts with sodium hydroxide to form sodium carbonate and water. When 2.41 L of Carbon dioxide gas and 3.50 grams of Sodium hydroxide are reacted together in a lab, 4.75 grams of Sodium carbonate is produced.**
\[
\text{CO}_2(\text{g
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