Zusammenfassung der Ressource
Electrochemistry
- Galvanic Cells
Anmerkungen:
- http://www.youtube.com/watch?v=C26pH8kC_Wk
- Consist of two half cells
- Electrode immersed in electrolyte
- Through which ions move
- Connected to each other by a wire
- Through which electrons move
- Each electrolyte is connected by a salt bridge
- Through which ions move
- Oxidation / Reduction
- Oxidation
- Occurs at Anode
- Occurs at negative terminal
- Reduction
- Occurs at Cathode
- Occurs at positive terminal
- Galvanic Cell
- Reactions
- Anode
- Zn -> Zn2+ + 2e-
- Cathode
- Cu2+ + 2e- -> Cu
- Electrons travel through circuit in order to reach other half cell
- The more reactive metal will always give electrons
- The less reactive metal will always take electrons
- Rechargeable Cells
- Fuel Cells
- How they work
- Use Hydrogen and Oxygen
- Split hydrogen electrons from protons
- Then join them up on other side of curcuit
- Produce only water
- Positives
- Produce no harmful waste products
- Can theoretically go forever
- Allow us to attain power in far off locations
- Negatives
- Very Expensive
- Electrolytic Cells
- Lead Car Battery
- Recharge through electrolysis
- Works like galvanic cell
- Recharging
- Lead Electrode:
Pb2+ + 2e- → Pb
- Lead Oxide Electrode:
Pb2+ → Pb4+ + 2e-