Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese (IV) oxide. 4 HCl(aq) + MnO₂ (s) → MnCl₂ (aq) + 2 H₂O(l) + Cl₂(g) A sample of 42.5 g MnO₂ is added to a solution containing 50.9 g HC1. What is the limiting reactant? MnO₂ HC1 What is the theoretical yield of Cl₂? theoretical yield: If the yield of the reaction is 84.1%, what is the actual yield of chlorine? actual yield: g Cl₂ g Cl₂
Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese (IV) oxide. 4 HCl(aq) + MnO₂ (s) → MnCl₂ (aq) + 2 H₂O(l) + Cl₂(g) A sample of 42.5 g MnO₂ is added to a solution containing 50.9 g HC1. What is the limiting reactant? MnO₂ HC1 What is the theoretical yield of Cl₂? theoretical yield: If the yield of the reaction is 84.1%, what is the actual yield of chlorine? actual yield: g Cl₂ g Cl₂
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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![**Chemical Reaction and Calculation of Yield in Chlorine Gas Production**
Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide.
\[ \text{4 HCl(aq) + MnO}_2\text{(s) } \rightarrow \text{ MnCl}_2\text{(aq) + 2 H}_2\text{O(l) + Cl}_2\text{(g)} \]
A sample of 42.5 g of MnO₂ is added to a solution containing 50.9 g of HCl.
**Questions and Calculations:**
1. **What is the limiting reactant?**
- **Options:**
- MnO₂
- HCl
2. **What is the theoretical yield of Cl₂?**
- Theoretical yield: ______ g Cl₂
3. **Actual Yield Calculation:**
- If the yield of the reaction is 84.1%, what is the actual yield of chlorine?
- Actual yield: ______ g Cl₂
**Instructions:**
- Determine the limiting reactant by comparing the mole ratio of the reactants.
- Calculate the theoretical yield based on stoichiometric calculations.
- Compute the actual yield using the given percentage yield formula:
\[
\text{Actual Yield} = \left(\frac{\text{Percentage Yield}}{100}\right) \times \text{Theoretical Yield}
\]
Provide your answers in the spaces provided.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd2659b4c-30a6-48d4-90ed-e5c7a02f7b8e%2F24c48d62-e6d7-47d3-8c4b-ef1fbe527618%2Fefu5vlg_processed.png&w=3840&q=75)
Transcribed Image Text:**Chemical Reaction and Calculation of Yield in Chlorine Gas Production**
Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide.
\[ \text{4 HCl(aq) + MnO}_2\text{(s) } \rightarrow \text{ MnCl}_2\text{(aq) + 2 H}_2\text{O(l) + Cl}_2\text{(g)} \]
A sample of 42.5 g of MnO₂ is added to a solution containing 50.9 g of HCl.
**Questions and Calculations:**
1. **What is the limiting reactant?**
- **Options:**
- MnO₂
- HCl
2. **What is the theoretical yield of Cl₂?**
- Theoretical yield: ______ g Cl₂
3. **Actual Yield Calculation:**
- If the yield of the reaction is 84.1%, what is the actual yield of chlorine?
- Actual yield: ______ g Cl₂
**Instructions:**
- Determine the limiting reactant by comparing the mole ratio of the reactants.
- Calculate the theoretical yield based on stoichiometric calculations.
- Compute the actual yield using the given percentage yield formula:
\[
\text{Actual Yield} = \left(\frac{\text{Percentage Yield}}{100}\right) \times \text{Theoretical Yield}
\]
Provide your answers in the spaces provided.
Expert Solution
Step 1
Given,
4HCl(aq) + MnO2(s) → MnCl2(aq) + 2H2O(l) + Cl2(g)
mass of MnO2 reacts = 42.5 g
nass of HCl reacts = 50.9 g
a) Limiting reactant = ?
b) Theoretical yield of Cl2 = ?
c) Actual yield of Chlorine = ?
Note:
molar mass of MnO2 = 86.9368 g/mol
molar mass of HCl = 36.458 g/mol
molar mass of Cl2 = 70.906 g/mol
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