Learning Goal: To understand the components and processes of a galvanic cell. A galvanic cell (or voltaic cell) produces electricity using a spontaneous redox reaction, such as the one shown here: Ni(s) + Cu²+ (aq) Ni²+ (aq) + Cu(s) The components of this reaction are separated by a salt bridge and connected with a wire, forcing the electrons to travel across the wire, creating electricity. Ni Ni² (aq) salt bridge Cu Cu (aq) The salt bridge is a U-shaped glass tube that is filled with a gel-like substance containing a salt. The salt bridge completes the circuit and allows ions to flow. maintaining electrical neutrality in the solutions. Part A Describe the electrodes in this nickel-copper galvanic cell. Drag the appropriate items to their respective bins. ▸ View Available Hint(s) Nickel anode cathode gains mass Copper loses mass Reset Help
Learning Goal: To understand the components and processes of a galvanic cell. A galvanic cell (or voltaic cell) produces electricity using a spontaneous redox reaction, such as the one shown here: Ni(s) + Cu²+ (aq) Ni²+ (aq) + Cu(s) The components of this reaction are separated by a salt bridge and connected with a wire, forcing the electrons to travel across the wire, creating electricity. Ni Ni² (aq) salt bridge Cu Cu (aq) The salt bridge is a U-shaped glass tube that is filled with a gel-like substance containing a salt. The salt bridge completes the circuit and allows ions to flow. maintaining electrical neutrality in the solutions. Part A Describe the electrodes in this nickel-copper galvanic cell. Drag the appropriate items to their respective bins. ▸ View Available Hint(s) Nickel anode cathode gains mass Copper loses mass Reset Help
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section: Chapter Questions
Problem 94QRT: An electrolytic cell is set up with Cd(s) in Cd(NO3)2(aq) and Zn(s) in Zn(NO3)2(aq). Initially both...
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![**Introduction to Galvanic Cells**
**Learning Goal:**
To understand the components and processes of a galvanic cell.
A galvanic cell (or voltaic cell) produces electricity using a spontaneous redox reaction, such as the one shown here:
Ni(s) + Cu²⁺(aq) → Ni²⁺(aq) + Cu(s)
The components of this reaction are separated by a salt bridge and connected with a wire, forcing the electrons to travel across the wire, creating electricity.
**Diagram Description:**
The diagram shows a U-shaped glass tube salt bridge connecting two beakers. Each beaker contains an electrode and a solution:
- The left beaker has a Nickel (Ni) electrode in a Ni²⁺(aq) solution.
- The right beaker has a Copper (Cu) electrode in a Cu²⁺(aq) solution.
The salt bridge is filled with a gel-like substance containing a salt. It completes the circuit and allows ions to flow, maintaining electrical neutrality in the solutions.
**Part A**
Describe the electrodes in this nickel-copper galvanic cell.
Drag the appropriate items to their respective bins.
- Available words: anode, cathode, gains mass, loses mass
**Nickel Box**
- [ ]
**Copper Box**
- [ ]
**Buttons:**
- Reset
- Help
**Submit**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F02dc2c71-84ec-4756-9bbf-6d095e097774%2F8073faf6-290f-4272-9aad-e5c9d98659a1%2F3c2zicn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Introduction to Galvanic Cells**
**Learning Goal:**
To understand the components and processes of a galvanic cell.
A galvanic cell (or voltaic cell) produces electricity using a spontaneous redox reaction, such as the one shown here:
Ni(s) + Cu²⁺(aq) → Ni²⁺(aq) + Cu(s)
The components of this reaction are separated by a salt bridge and connected with a wire, forcing the electrons to travel across the wire, creating electricity.
**Diagram Description:**
The diagram shows a U-shaped glass tube salt bridge connecting two beakers. Each beaker contains an electrode and a solution:
- The left beaker has a Nickel (Ni) electrode in a Ni²⁺(aq) solution.
- The right beaker has a Copper (Cu) electrode in a Cu²⁺(aq) solution.
The salt bridge is filled with a gel-like substance containing a salt. It completes the circuit and allows ions to flow, maintaining electrical neutrality in the solutions.
**Part A**
Describe the electrodes in this nickel-copper galvanic cell.
Drag the appropriate items to their respective bins.
- Available words: anode, cathode, gains mass, loses mass
**Nickel Box**
- [ ]
**Copper Box**
- [ ]
**Buttons:**
- Reset
- Help
**Submit**
![**Standard Reduction Potentials for Nickel(II) and Copper(II)**
The standard reduction potential for a substance indicates how readily that substance gains electrons relative to other substances at standard conditions. The more positive the reduction potential, the more easily the substance gains electrons. Consider the following reactions:
1. \( \text{Ni}^{2+} (aq) + 2e^- \rightarrow \text{Ni}(s) \), with a standard reduction potential \( E^\circ_\text{red} = -0.230 \, \text{V} \)
2. \( \text{Cu}^{2+} (aq) + 2e^- \rightarrow \text{Cu}(s) \), with a standard reduction potential \( E^\circ_\text{red} = +0.337 \, \text{V} \)
---
**Part B**
**Question:** What is the standard potential, \( E^\circ_\text{cell} \), for this galvanic cell? Use the given standard reduction potentials in your calculation as appropriate.
Express your answer to three decimal places and include the appropriate units.
[Option to view available hint(s)]
**Answer Box:**
\( E^\circ_\text{cell} = \) [Value] [Units]
**Submit Button:** Submit
---
**Explanation:**
- The image presents two standard reduction potentials for nickel and copper, which indicate their tendencies to gain electrons in chemical reactions.
- Students are tasked with calculating the standard cell potential for a galvanic cell using the provided reduction potentials.
- The format requires users to express the answer with precision and specify the correct units.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F02dc2c71-84ec-4756-9bbf-6d095e097774%2F8073faf6-290f-4272-9aad-e5c9d98659a1%2Fin86xfg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Standard Reduction Potentials for Nickel(II) and Copper(II)**
The standard reduction potential for a substance indicates how readily that substance gains electrons relative to other substances at standard conditions. The more positive the reduction potential, the more easily the substance gains electrons. Consider the following reactions:
1. \( \text{Ni}^{2+} (aq) + 2e^- \rightarrow \text{Ni}(s) \), with a standard reduction potential \( E^\circ_\text{red} = -0.230 \, \text{V} \)
2. \( \text{Cu}^{2+} (aq) + 2e^- \rightarrow \text{Cu}(s) \), with a standard reduction potential \( E^\circ_\text{red} = +0.337 \, \text{V} \)
---
**Part B**
**Question:** What is the standard potential, \( E^\circ_\text{cell} \), for this galvanic cell? Use the given standard reduction potentials in your calculation as appropriate.
Express your answer to three decimal places and include the appropriate units.
[Option to view available hint(s)]
**Answer Box:**
\( E^\circ_\text{cell} = \) [Value] [Units]
**Submit Button:** Submit
---
**Explanation:**
- The image presents two standard reduction potentials for nickel and copper, which indicate their tendencies to gain electrons in chemical reactions.
- Students are tasked with calculating the standard cell potential for a galvanic cell using the provided reduction potentials.
- The format requires users to express the answer with precision and specify the correct units.
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