Part B What are the coefficients of the reactants and products in the balanced equation above? Remember to include H₂O(1) and OH-(aq) in the blanks where appropriate. Your answer should have six terms. Enter the equation coefficients in order separated by commas (e.g., 2,2,1,4,4,3). Include coefficients of 1, as required, for grading purposes. ▸ View Available Hint(s)
Part B What are the coefficients of the reactants and products in the balanced equation above? Remember to include H₂O(1) and OH-(aq) in the blanks where appropriate. Your answer should have six terms. Enter the equation coefficients in order separated by commas (e.g., 2,2,1,4,4,3). Include coefficients of 1, as required, for grading purposes. ▸ View Available Hint(s)
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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Question
![**Basic Solution**
Potassium permanganate, \( \text{KMnO}_4 \), is a powerful oxidizing agent. The products of a given redox reaction with the permanganate ion depend on the reaction conditions used. In basic solution, the following equation represents the reaction of this ion with a solution containing sodium fluoride:
\[
\text{MnO}_4^- \, (aq) + \text{F}^- \, (aq) \rightarrow \text{MnO}_2 \, (s) + \text{F}_2 \, (aq)
\]
Since this reaction takes place in a basic solution, \( \text{H}_2\text{O}(l) \) and \( \text{OH}^- \, (aq) \) will be shown in the reaction. Places for these species are indicated by the blanks in the following restatement of the equation:
\[
\text{MnO}_4^- \, (aq) + \text{F}^- \, (aq) + \_\_\_ \rightarrow \text{MnO}_2 \, (s) + \text{F}_2 \, (aq) + \_\_\_
\]
**Part B**
What are the coefficients of the reactants and products in the balanced equation above? Remember to include \( \text{H}_2\text{O}(l) \) and \( \text{OH}^- \, (aq) \) in the blanks where appropriate. Your answer should have six terms.
Enter the equation coefficients in order separated by commas (e.g., 2, 2, 1, 4, 4, 3). Include coefficients of 1, as required, for grading purposes.
**[View Available Hint(s)]**
[Textbox for coefficients input]
[Submit Button]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F02dc2c71-84ec-4756-9bbf-6d095e097774%2F870fe7ba-99bd-4479-ba0f-9583edc964b5%2F4lnbl9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Basic Solution**
Potassium permanganate, \( \text{KMnO}_4 \), is a powerful oxidizing agent. The products of a given redox reaction with the permanganate ion depend on the reaction conditions used. In basic solution, the following equation represents the reaction of this ion with a solution containing sodium fluoride:
\[
\text{MnO}_4^- \, (aq) + \text{F}^- \, (aq) \rightarrow \text{MnO}_2 \, (s) + \text{F}_2 \, (aq)
\]
Since this reaction takes place in a basic solution, \( \text{H}_2\text{O}(l) \) and \( \text{OH}^- \, (aq) \) will be shown in the reaction. Places for these species are indicated by the blanks in the following restatement of the equation:
\[
\text{MnO}_4^- \, (aq) + \text{F}^- \, (aq) + \_\_\_ \rightarrow \text{MnO}_2 \, (s) + \text{F}_2 \, (aq) + \_\_\_
\]
**Part B**
What are the coefficients of the reactants and products in the balanced equation above? Remember to include \( \text{H}_2\text{O}(l) \) and \( \text{OH}^- \, (aq) \) in the blanks where appropriate. Your answer should have six terms.
Enter the equation coefficients in order separated by commas (e.g., 2, 2, 1, 4, 4, 3). Include coefficients of 1, as required, for grading purposes.
**[View Available Hint(s)]**
[Textbox for coefficients input]
[Submit Button]
![**Week 6 Assignment: Electrochemistry**
**Balancing Redox Equations: Half-reaction Method**
In addition to mass balance, oxidation-reduction reactions must be balanced such that the number of electrons lost in the oxidation equals the number of electrons gained in the reduction. This balancing can be done by two methods: the half-reaction method or the oxidation number method. The half-reaction method balances the electrons lost in the oxidation half-reaction with the electrons gained in the reduction half-reaction. In either method, H₂O(l), OH⁻(aq), and H⁺(aq) may be added to complete the mass balance. Which substances are used depends on the reaction conditions.
**Acidic solution**
In acidic solution, the sulfate ion can be used to react with a number of metal ions. One such reaction is:
\[ \text{SO}_3^{2-} \, (aq) + \text{Sn}^{4+} \, (aq) \rightarrow \text{H}_2\text{SO}_3 \, (aq) + \text{Sn}^{2+} \, (aq) \]
Since this reaction takes place in acidic solution, H₂O(l) and H⁺(aq) will be involved in the reaction. Places for these species are indicated by the blanks in the following restatement of the equation:
\[ \text{SO}_3^{2-} \, (aq) + \text{Sn}^{4+} \, (aq) + \ldots \rightarrow \text{H}_2\text{SO}_3 \, (aq) + \text{Sn}^{2+} \, (aq) + \ldots \]
**Part A**
What are the coefficients of the reactants and products in the balanced equation above? Remember to include H₂O(l) and H⁺(aq) in the appropriate blanks. Your answer should have six terms.
Enter the equation coefficients in order separated by commas (e.g., 2, 2, 1, 4, 4, 3). Include coefficients of 1, as required, for grading purposes.
- [View Available Hint(s)]
- [Submit]
**Basic solution**
Potassium permanganate, KMnO₄, is a powerful oxidizing agent. The products of a given redox reaction with the permanganate ion depend on the](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F02dc2c71-84ec-4756-9bbf-6d095e097774%2F870fe7ba-99bd-4479-ba0f-9583edc964b5%2Fwl94vkg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Week 6 Assignment: Electrochemistry**
**Balancing Redox Equations: Half-reaction Method**
In addition to mass balance, oxidation-reduction reactions must be balanced such that the number of electrons lost in the oxidation equals the number of electrons gained in the reduction. This balancing can be done by two methods: the half-reaction method or the oxidation number method. The half-reaction method balances the electrons lost in the oxidation half-reaction with the electrons gained in the reduction half-reaction. In either method, H₂O(l), OH⁻(aq), and H⁺(aq) may be added to complete the mass balance. Which substances are used depends on the reaction conditions.
**Acidic solution**
In acidic solution, the sulfate ion can be used to react with a number of metal ions. One such reaction is:
\[ \text{SO}_3^{2-} \, (aq) + \text{Sn}^{4+} \, (aq) \rightarrow \text{H}_2\text{SO}_3 \, (aq) + \text{Sn}^{2+} \, (aq) \]
Since this reaction takes place in acidic solution, H₂O(l) and H⁺(aq) will be involved in the reaction. Places for these species are indicated by the blanks in the following restatement of the equation:
\[ \text{SO}_3^{2-} \, (aq) + \text{Sn}^{4+} \, (aq) + \ldots \rightarrow \text{H}_2\text{SO}_3 \, (aq) + \text{Sn}^{2+} \, (aq) + \ldots \]
**Part A**
What are the coefficients of the reactants and products in the balanced equation above? Remember to include H₂O(l) and H⁺(aq) in the appropriate blanks. Your answer should have six terms.
Enter the equation coefficients in order separated by commas (e.g., 2, 2, 1, 4, 4, 3). Include coefficients of 1, as required, for grading purposes.
- [View Available Hint(s)]
- [Submit]
**Basic solution**
Potassium permanganate, KMnO₄, is a powerful oxidizing agent. The products of a given redox reaction with the permanganate ion depend on the
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