Complete and balance the following redox reaction in basic solution. Be sure to include the proper phases for all species within the reaction. 2- MnO4 (aq) + C₂O4² (aq) → MnO₂(s) + CO₂(g)
Complete and balance the following redox reaction in basic solution. Be sure to include the proper phases for all species within the reaction. 2- MnO4 (aq) + C₂O4² (aq) → MnO₂(s) + CO₂(g)
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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![### Balancing Redox Reactions in Basic Solution
#### Question 10 of 40
**Objective:** Complete and balance the following redox reaction in a basic solution. Ensure to include the appropriate phases for all species involved in the reaction.
**Unbalanced Reaction:**
\[ \text{MnO}_{4}^{-} (aq) + \text{C}_{2}\text{O}_{4}^{2-} (aq) \rightarrow \text{MnO}_{2} (s) + \text{CO}_{2} (g) \]
**Interface Explanation:**
- **3C\(_2\)2\(^{-}\):** A button to use specific coefficients or subscripts, possibly related to oxalate ion (C\(_2\)O\(_4\)\(^{2-}\)).
- **Reset Button:** Clears current inputs or selections in the balancing process.
- **Directional Arrows (<, >):** Navigate through steps or options in the equation editor.
- **Numerals (0-9):** Enter specific numbers required for coefficients in the balanced equation.
- **Operators (+, -, →, ⇌):** Include reaction specifics, such as reactants, products, and equilibrium processes.
- **Phase Labels ((s), (l), (g), (aq)):** Indicate the physical states of chemicals: solid (s), liquid (l), gas (g), aqueous (aq).
- **Chemical Components:** Buttons to include ions or molecules such as C, H\(^+\), H\(_2\)O, Mn, e\(^{-}\), H\(_3\)O\(^+\), H, OH\(^{-}\), O, and water hydration factors (\(\cdot x \text{H}_2\text{O}\)).
This question asks students to skillfully apply knowledge of redox reactions and balance them, highlighting important skills in stoichiometry and chemical phase notation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa8099e47-3d0e-448d-afd1-356c22244100%2F942c895c-7c27-4aad-a262-c457a885460c%2Fcn8to7_processed.png&w=3840&q=75)
Transcribed Image Text:### Balancing Redox Reactions in Basic Solution
#### Question 10 of 40
**Objective:** Complete and balance the following redox reaction in a basic solution. Ensure to include the appropriate phases for all species involved in the reaction.
**Unbalanced Reaction:**
\[ \text{MnO}_{4}^{-} (aq) + \text{C}_{2}\text{O}_{4}^{2-} (aq) \rightarrow \text{MnO}_{2} (s) + \text{CO}_{2} (g) \]
**Interface Explanation:**
- **3C\(_2\)2\(^{-}\):** A button to use specific coefficients or subscripts, possibly related to oxalate ion (C\(_2\)O\(_4\)\(^{2-}\)).
- **Reset Button:** Clears current inputs or selections in the balancing process.
- **Directional Arrows (<, >):** Navigate through steps or options in the equation editor.
- **Numerals (0-9):** Enter specific numbers required for coefficients in the balanced equation.
- **Operators (+, -, →, ⇌):** Include reaction specifics, such as reactants, products, and equilibrium processes.
- **Phase Labels ((s), (l), (g), (aq)):** Indicate the physical states of chemicals: solid (s), liquid (l), gas (g), aqueous (aq).
- **Chemical Components:** Buttons to include ions or molecules such as C, H\(^+\), H\(_2\)O, Mn, e\(^{-}\), H\(_3\)O\(^+\), H, OH\(^{-}\), O, and water hydration factors (\(\cdot x \text{H}_2\text{O}\)).
This question asks students to skillfully apply knowledge of redox reactions and balance them, highlighting important skills in stoichiometry and chemical phase notation.
![**Redox Reaction Balancing in Acidic Solution**
**Question 9 of 40**
**Task:** Complete and balance the following redox reaction in an acidic solution. Be sure to include the proper phases for all species within the reaction.
\[ \text{BiO}_3^- (aq) + \text{S}_2\text{O}_3^{2-} (aq) \rightarrow \text{Bi}^{3+} (aq) + \text{S}_4\text{O}_6^{2-} (aq) \]
**Instructions:**
- Use the appropriate tools below to balance the chemical equation.
- Note that the available elements and ions can be selected from the panel.
- Options to modify the equation include digits, basic arithmetic signs, phases of matter, and chemical species identifiers.
**Explanation:**
This exercise involves balancing a redox (reduction-oxidation) reaction in an acidic environment. The initial reagents and final products are given, including their respective aqueous (aq) states. The goal is to balance the number of atoms and charge on both sides of the equation, making use of the given tools like ions, water, and protons.
**Tips for Balancing:**
1. **Identify Oxidation and Reduction Parts:**
- Determine which elements are being oxidized and reduced.
2. **Balance Atoms:**
- Balance the atoms for each half-reaction.
3. **Charge Balance:**
- Add electrons (e⁻) to balance the charges.
4. **Combine Half-Reactions:**
- Ensure both sides have equal numbers of electrons, then combine the half-reactions.
5. **Check Phases and Charges:**
- Verify that the number of atoms and charges are equal on both sides.
This practice will enhance understanding of redox reactions, particularly in how they are balanced in acidic conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa8099e47-3d0e-448d-afd1-356c22244100%2F942c895c-7c27-4aad-a262-c457a885460c%2F2m899g_processed.png&w=3840&q=75)
Transcribed Image Text:**Redox Reaction Balancing in Acidic Solution**
**Question 9 of 40**
**Task:** Complete and balance the following redox reaction in an acidic solution. Be sure to include the proper phases for all species within the reaction.
\[ \text{BiO}_3^- (aq) + \text{S}_2\text{O}_3^{2-} (aq) \rightarrow \text{Bi}^{3+} (aq) + \text{S}_4\text{O}_6^{2-} (aq) \]
**Instructions:**
- Use the appropriate tools below to balance the chemical equation.
- Note that the available elements and ions can be selected from the panel.
- Options to modify the equation include digits, basic arithmetic signs, phases of matter, and chemical species identifiers.
**Explanation:**
This exercise involves balancing a redox (reduction-oxidation) reaction in an acidic environment. The initial reagents and final products are given, including their respective aqueous (aq) states. The goal is to balance the number of atoms and charge on both sides of the equation, making use of the given tools like ions, water, and protons.
**Tips for Balancing:**
1. **Identify Oxidation and Reduction Parts:**
- Determine which elements are being oxidized and reduced.
2. **Balance Atoms:**
- Balance the atoms for each half-reaction.
3. **Charge Balance:**
- Add electrons (e⁻) to balance the charges.
4. **Combine Half-Reactions:**
- Ensure both sides have equal numbers of electrons, then combine the half-reactions.
5. **Check Phases and Charges:**
- Verify that the number of atoms and charges are equal on both sides.
This practice will enhance understanding of redox reactions, particularly in how they are balanced in acidic conditions.
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Follow-up Questions
Read through expert solutions to related follow-up questions below.
Follow-up Question
Your submitted reaction is unbalanced. In your reaction, there are 20 oxygen, 1
manganese atoms in the reactants but 24 oxygen, 2 manganese atoms in the products. Reconsider the coefficients in front of your reactants and/or products and try again. The following steps may help you balance this
- Split the given equation into two half-reactions: one for oxidation and one for reduction
- For each half-reaction, balance all atoms except H and O on both sides of the equation by altering the coefficients.
-
- Balance O by adding H2O to the appropriate side of the equations as needed
- After adding H2O, balance H by adding
H+ to the appropriate side of the equation as needed
- Determine the number of electrons (e) lost or gained in each half-reaction and add e to the appropriate side of the equations to balance charge.
- Add OH to both sides of the equation to neutralize all of the H* by forming H2O
- Cancel out water molecules that appear as both reactants and products
- Multiply each half-reaction by whole numbers as needed to make the same number of electrons appear in both half-reactions
- Add the two half-reactions and ensure that electrons completely cancel out.
- Simplify the equation by cancelling out species that appear on both sides.
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