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1. Assignment chemistry 2024-2025 Electochemistry Galvanic cells t.s.surya siddharth Xii-d by

2. 1.Introduction 2.Basic Components of a Galvanic Cell 3.Working Principle 4.Standard Electrode Potentials 5.Nernst Equation 6.Example: Zinc-Copper Galvanic Cell 7.Sample Problems 8.Applications of Galvanic Cells 9.Conclusion 10.References Table of Contents

3. Basic Components of a Galvanic Cell Electrodes : These are solid conductors where the oxidation and reduction reactions occur . Anode : Where oxidation takes place . Cathode : Where reduction occurs . Salt Bridge : A medium that allows ions to flow between the two half-cells while preventing direct mixing of the solutions . Electrolyte : An ionic solution that facilitates the transfer of charge by moving ions to the electrodes . External Circuit : The path that electrons follow, traveling from the anode to the cathode.

4. Diagram of a Galvanic Cell:

5. 2. Working Principle The working of a Galvanic cell is based on the following steps : Oxidation occurs at the anode (negative terminal), causing a loss of electrons . Reduction occurs at the cathode (positive terminal), Where electrons are gained . Electrons travel through the external circuit from the anode to the cathode, generating an electric current . The salt bridge completes the circuit by balancing the charge as ions move between the two half-cells.

6. Standard Electrode Potentials The Standard Electrode Potential (E°) is the potential difference between an electrode and its solution at standard conditions (1M concentration, 298 K temperature , and 1 atm pressure). The potential of a galvanic cell is the difference between the reduction potentials of the cathode and anode: E° cell ​= E° cathode − E° anode ​ Reaction E ∘ (V) Zn 2+ +2e − → Zn(s) -0.76 Cu 2+ +2e − → Cu(s) +0.34 Standard Electrode Potentials (Examples):

7. 4. Nernst Equation The Nernst Equation allows us to calculate the potential of a Galvanic cell under non-standard conditions. The equation is: E=E ∘ −(0.0592/n ) log([reactants]/[products]​) Where : E is the cell potential . E ∘ is the standard cell potential . n is the number of moles of electrons transferred . []represents the concentrations of ions.

8. 5. Example: Zinc-Copper Galvanic Cell In a Zinc-Copper Cell : Anode : Zinc is oxidized . Zn(s )→Zn 2 +( aq )+2e − Cathode : Copper is reduced . Cu 2 + ( aq )+2e − → Cu(s) The overall cell reaction : Zn(s )+Cu 2+ ( aq )→ Zn 2+ ( aq )+ Cu(s) The standard cell potential : E ∘ cell =( 0.34 V)−(−0.76 V)=1.10  V

9. 6. Sample Problems Problem 1 : Calculate the standard cell potential for a Galvanic cell made of magnesium (Mg) and silver (Ag), given : Mg 2 + +2e − → Mg(s), E ∘ =−2.37  V Ag + +e − → Ag(s),E ∘ =+ 0.80V Solution : E ∘ cell =( 0.80 V)−(−2.37 V)=3.17  V E° cell ​= E° cathode − E° anode ​

10. 7. Applications of Galvanic Cells Batteries : Galvanic cells are the fundamental building blocks of most batteries. Corrosion Prevention : Galvanic cells help in understanding corrosion processes and developing prevention techniques like galvanizing . Electroplating : In industries, the electrochemical principles of Galvanic cells are used to coat objects with metals.

11. 8. Conclusion Galvanic cells play a crucial role in many practical applications by converting chemical energy into electrical energy. By understanding their basic components, working principles, and applications, one can grasp the foundational concepts of electrochemistry and its importance in everyday life.

12. 9. References Atkins, P., & de Paula, J. (2013). Physical Chemistry (10th ed.). Oxford University Press . Bard, A. J., & Faulkner, L. R. (2001). Electrochemical Methods: Fundamentals and Applications . Wiley . Petrucci , R. H., Herring, F. G., Madura, J. D., & Bissonnette , C. (2017 ). General Chemistry: Principles and Modern Applications (11th ed .). Pearson .