### Electrochemical Reactions Worksheet**Instructions:**- Please provide balanced equations for the reactions described below.- Ensure each equation is balanced in terms of mass and charge.---**1. Write a balanced equation for the half-reaction that happens at the cathode.**| Reaction | ||----------|----------|| | |---**2. Write a balanced equation for the half-reaction that happens at the anode.**| Reaction | ||----------|----------|| | |---**3. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.**| Reaction | ||----------|----------|| | | --- *Note:* Each equation should include the appropriate states of matter (solid, liquid, aqueous, gas) and ensure the correct stoichiometric coefficients are used to balance the equation.---This worksheet is designed to aid in understanding and practicing the balancing of electrochemical reactions, including both half-reactions at the cathode and anode, and the overall spontaneous reaction that occurs in an electrochemical cell. ### Galvanic Cell DesignA chemist designs a galvanic cell that uses these two half-reactions:| half-reaction | standard reduction potential || -------------------------------------------- | ------------------------------------ || \( 2 \text{IO}_3^- (aq) + 12 \text{H}^+ (aq) + 10 e^- \rightarrow \text{I}_2 (s) + 6 \text{H}_2 \text{O} (l) \) | \( E^0_{\text{red}} = +1.195 \, \text{V} \) || \( \text{Cl}_2 (g) + 2 e^- \rightarrow 2 \text{Cl}^- (aq) \) | \( E^0_{\text{red}} = +1.359 \, \text{V} \) |This table outlines the half-reactions along with their standard reduction potentials (\( E^0_{\text{red}} \)) in volts. In a galvanic cell, these potentials help determine which reactions will occur at the anode and cathode, thus pointing to the overall cell potential.

Two half cell reactions of a galvanic cell are given.

Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.

Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.

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

### Electrochemical Reactions Worksheet

**Instructions:**
- Please provide balanced equations for the reactions described below.
- Ensure each equation is balanced in terms of mass and charge.

---

**1. Write a balanced equation for the half-reaction that happens at the cathode.**

| Reaction | |
|----------|----------|
| | |

---

**2. Write a balanced equation for the half-reaction that happens at the anode.**

| Reaction | |
|----------|----------|
| | |

---

**3. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.**

| Reaction | |
|----------|----------|
| | |

---

*Note:* Each equation should include the appropriate states of matter (solid, liquid, aqueous, gas) and ensure the correct stoichiometric coefficients are used to balance the equation.

---

This worksheet is designed to aid in understanding and practicing the balancing of electrochemical reactions, including both half-reactions at the cathode and anode, and the overall spontaneous reaction that occurs in an electrochemical cell.

### Galvanic Cell Design

A chemist designs a galvanic cell that uses these two half-reactions:

| half-reaction | standard reduction potential |
| -------------------------------------------- | ------------------------------------ |
| \( 2 \text{IO}_3^- (aq) + 12 \text{H}^+ (aq) + 10 e^- \rightarrow \text{I}_2 (s) + 6 \text{H}_2 \text{O} (l) \) | \( E^0_{\text{red}} = +1.195 \, \text{V} \) |
| \( \text{Cl}_2 (g) + 2 e^- \rightarrow 2 \text{Cl}^- (aq) \) | \( E^0_{\text{red}} = +1.359 \, \text{V} \) |

This table outlines the half-reactions along with their standard reduction potentials (\( E^0_{\text{red}} \)) in volts. In a galvanic cell, these potentials help determine which reactions will occur at the anode and cathode, thus pointing to the overall cell potential.

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