📳📶AGalvanic Cell
📶📳A galvanic cell, also known as a voltaic cell, is an electrochemical cell that converts chemical energy into electrical energy through spontaneous redox (oxidation-reduction) reactions. Here’s a breakdown of its components and how it operates:
📶📳Components of a Galvanic Cell:
1. 📶📳Electrodes**:
- **Anode**: The electrode where oxidation occurs (loss of electrons). It is negatively charged in a galvanic cell.
- **Cathode**: The electrode where reduction occurs (gain of electrons). It is positively charged in a galvanic cell.
2. 📳📶Electrolyte**: A solution that conducts electricity, containing ions that participate in the redox reaction.
3. 📳📶Salt Bridge**: Often a tube filled with a gel-like electrolyte, it connects the two half-cells and allows ions to flow between them while preventing the solutions from mixing completely. This maintains charge balance.
📶📳 Working Principle:
1. 📳Oxidation** occurs at the anode, releasing electrons. For example, if zinc is used:
\[
\text{Zn} \rightarrow \text{Zn}^{2+} + 2e^-
\]
2.📳 The released electrons travel through the external circuit to the cathode.
3. 📳Reduction** occurs at the cathode, where the electrons are accepted. For example, in the case of copper ions:
\[
\text{Cu}^{2+} + 2e^- \rightarrow \text{Cu}
\]
4. 📳📶The flow of electrons from the anode to the cathode generates electric current.
📶📳#Applications:
- Galvanic cells are used in batteries, where they provide power for various devices, from small electronics to electric vehicles.
- They are also crucial in chemical sensing and electroplating.
#📳📶Example:
A common example of a galvanic cell is the Daniel cell, which consists of a zinc electrode in a zinc sulfate solution (anode) and a copper electrode in a copper sulfate solution (cathode).
📶📳 Key Equations:
📳📶Nernst Equation**: Used to calculate the cell potential under non-standard conditions.
📶📳Cell Potential (\(E\))**: Given by the difference between the reduction potentials of the cathode and anode.
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