🔹 Unit 1: Electrochemistry & Battrychemistry🔹

🔹 Electrochemistry : A branch of science that explores the connection between electrical current and chemical reactions, linking them together.  - Looking ahead, 🧪Electrochemical cells are classified into two main types:                                                                  🌿🔋Electrolytic cells  &  ⚗️Galvanic cells.                                                                                   🔋 Electrolytic Cell 🔋 🔋 Electrolytic cell : -  Electrolytic cell is a device which converts :                           ⚡️Electrical energy(from an external source) ➡️➡️🔋Chemical energy. -  An electrolytic cell contains 2 rods, also called electrodes⚗️.                             🌿These electrodes can be made of different metals or the same metal, like graphite or metallic ones. They are dipped in the same 🔬electrolytic solution.  - The electrode is linked to the battery🔋.   🌿One electrode connected to the positive terminal of the battery is called the Anode (+), marked with a positive sign.   🌿The other electrode connected to the negative terminal of the battery is known as the Cathode (-), bearing a negative sign. ⚡️🔋                                                                                ⚗️ Galvanic cell ⚗️                                                                                ⚗️ Galvanic cell :   -  Galvanic cell is a device which converts :                           🔋Chemical energy(of a redox reaction) ➡️➡️⚡Electrical energy. -  An Galvanic cell contains 2 rods, also called electrodes⚗️.                             🌿These electrodes(half cells) are made of different metals and are connected by salt bridge. They are dipped in different electrolytic solution respective  🔬electrolytic solution.  - The electrodes are connected to a potentiometer or voltmeter by an electrical wire. ⚡️ - The electrode where oxidation occurs is called :                                                     🌿Anode (Negative (-) Electrode). ⚗️ - The electrode where reduction occurs is called : also spontaneous redox reaction takes place on electrode                                                     🌿Cathode (Positive (+) Electrode). ⚡️                                                     🌿Example: Daniel cell 🔄 🌊Salt bridge & ⚖️Functions :  🌿 A salt bridge is like an upside-down U-tube filled with a strong electrolyte solution, such as                                                         💡KCl, KNO3, or NH4Cl.  🌿These electrolytes are chosen because the ions move at similar speeds, helping balance charges.  ⚖️Function of the Salt Bridge: 🌿Connects🔗 Half-Cells : Joins them to complete the circuit.  🌿Prevents Mixing🚫      : Stops solution movement between half-cells.  🌿Maintains Balance⚖️   : Keeps both halves electrically neutral.  🌿Prevents Potential Differences🛑: Stops liquid junction potential.  ⚡️ EMF of a Cell :  🌿When two electrodes connect, current moves from higher potential to lower potential. The difference in potential that drives this current is called the EMF of the cell. 🌿Ecell = E Cathode - E Anode   🌿Here, E cathode and E Anode are the reduction potentials of the cathode and anode, respectively.  🔹 Understanding Electrode Potential: 🌿When a metal meets its electrolytic solution, it picks up a charge, resulting in electrode potential. This reflects the metal's tendency to either lose or gain electrons.           ⚡️ Oxidation Potential: Metal's tendency to lose electrons.           ⚡️ Reduction Potential: Metal's tendency to gain electrons. 🔹Standard Electrode Potential:  🌿At a specific temp, it's a metal's tendency to oxidize or reduce when in contact with a 1M ion solution.     🌿SRP (Standard Reduction Potential): It's the tendency of a substance to undergo reduction.     🌿SOP (Standard Oxidation Potential): It's the tendency of a substance to undergo reduction. 🌟Thermodynamics of EMF of Cells  🧬Relationship between Enthalpy Change and EMF: 🌿Using the Gibbs-Helmholtz equation:                                    Combining equations (1) and (2): 🔹Nernst Equation & Its Derivation:  🌿The Nernst Equation helps us find cell or electrode potential in non-standard conditions. It connects the measured potential to the reaction quotient. 🔸Deriving the Equation: 🌿Consider a redox reaction: aA + bB → cC + dD .. make this in