Slide 1 of 12
Slide 1 - Zinc-Copper Cell Example Cell Potential & Notation
Zinc-Copper Cell Example Cell Potential & Notation
Notes on Electrochemical Principles
---
Photo by Stephan HK on Unsplash
Galvanic Cells: Zinc-Copper Example, Notation, and Cell Potential
Generated from prompt:
Write notes on galvanic cell, using zinc-copper cell as example. Determining the cell potential and cell notation
This presentation introduces galvanic cells, which generate electricity from spontaneous redox reactions. Using the classic zinc-copper cell as an example, it covers cell components, half-cell reactions (Zn oxidation at anode, Cu reduction at cathode), cell notation (Zn | Zn²⁺ || Cu²⁺ | Cu), standard reduction potentials, and cell potential calculation (E°_cell = 1.10 V). Includes agenda, diagrams, and key takeaways on electrochemical principles foundational to batteries.
May 13, 202612 slides
Slide 2 of 12
Slide 2 - Presentation Outline
- What is a Galvanic Cell?
- Zinc-Copper Cell Example
- Half-Cell Reactions
- Cell Notation
- Cell Potential Calculation
- Conclusion
---
Photo by Alfred Quartey on Unsplash
Slide 3 of 12
Slide 3 - Galvanic Cell Fundamentals
1
What is a Galvanic Cell
Generates electricity from spontaneous redox reactions
---
Photo by Ryan Zazueta on Unsplash
Slide 4 of 12
Slide 4 - Definition and Components
- Generates electric current from spontaneous oxidation–reduction (redox) reactions
- Two half-cells: each metal immersed in its respective metal ions solution
- Connected by salt bridge or porous membrane
- Named after Luigi Galvani and Alessandro Volta
- Example: Two different metals in separate beakers
Source: Wikipedia: Galvanic cell
Slide 5 of 12
Slide 5 - Zinc-Copper Example
Slide 6 of 12
Slide 6 - Zinc-Copper Galvanic Cell
- Zinc anode oxidizes: Zn → Zn²⁺ + 2e⁻
- Copper cathode reduces: Cu²⁺ + 2e⁻ → Cu
- Salt bridge maintains charge balance
- Electrons flow externally from anode to cathode
---
Photo by Claudio Schwarz on Unsplash
Slide 7 of 12
Slide 7 - Half-Cell Reactions
Anode (Oxidation) Zn(s) → Zn²⁺(aq) + 2e⁻ Less noble metal (Zn) loses electrons
Cathode (Reduction) Cu²⁺(aq) + 2e⁻ → Cu(s) More noble metal (Cu) gains electrons
Slide 8 of 12
Slide 8 - Cell Notation
- Convention: Anode | Anode²⁺(aq) || Cathode²⁺(aq) | Cathode
- Zinc-Copper: Zn(s) | Zn²⁺(aq) || Cu²⁺(aq) | Cu(s)
- | = phase boundary (solid|liquid)
- || = salt bridge or porous junction
- Anode on left (oxidation), cathode on right (reduction)
Slide 9 of 12
Slide 9 - Cell Potential
4
Determining Cell Potential
Using standard electrode potentials
---
Photo by Thorium on Unsplash
Slide 10 of 12
Slide 10 - Standard Reduction Potentials
| Electrode | Half-Reaction (Reduction) | E° (V) |
|---|---|---|
| Zn²⁺/Zn | Zn²⁺ + 2e⁻ → Zn | -0.76 |
| Cu²⁺/Cu | Cu²⁺ + 2e⁻ → Cu | +0.34 |
Source: Wikipedia: Galvanic series
Slide 11 of 12
Slide 11 - Calculating E_cell
- E°cell = E°cathode (reduction) - E°anode (reduction)
- E°cell = 0.34 V (Cu) - (-0.76 V) (Zn) = 1.10 V
- Positive E°_cell: spontaneous reaction
- Zinc (more negative potential) acts as anode
Source: Wikipedia: Galvanic series
Slide 12 of 12
Slide 12 - Key Takeaways
Galvanic Cell: Spontaneous redox generates electricity Zinc-Copper Example:
- Notation: Zn | Zn²⁺ || Cu²⁺ | Cu
- E°cell = 1.10 V (0.34 - (-0.76))
Foundation of batteries and electrochemical applications
---
Photo by Jorge Campos on Unsplash
Discover More Presentations
Explore thousands of AI-generated presentations for inspiration
Powered by AI
Create Your Own Presentation
Generate professional presentations in seconds with Karaf's AI. Customize this presentation or start from scratch.