What is the Standard electrod potential in chemistry class 12th

 

🔹 What is Standard Electrode Potential in Chemistry?

Standard Electrode Potential (denoted as ) is the electric potential (voltage) of a half-cell (electrode) measured under standard conditions when it is connected to the Standard Hydrogen Electrode (SHE), which is assigned a potential of 0.00 volts.


🔹 Definition:

Standard Electrode Potential (E°) is the potential developed by an electrode when it is in equilibrium with its ions at 1 M concentration, 1 atm pressure, and 25°C (298 K), compared to the Standard Hydrogen Electrode (SHE).


🔹 Standard Conditions:

  • Temperature = 25°C (298 K)
  • Concentration of ions = 1 M
  • Pressure of gases = 1 atm
  • Electrode connected to Standard Hydrogen Electrode (SHE)

🔹 Notation:

  • Represented as E°ₘ/ₘⁿ⁺ or E°(half-cell)
  • Measured in volts (V)

🔹 Example Values:

Electrode Half-cell Reaction E° (V)
Cu²⁺/Cu Cu²⁺ + 2e⁻ → Cu +0.34 V
Zn²⁺/Zn Zn²⁺ + 2e⁻ → Zn –0.76 V
H⁺/H₂ (SHE) 2H⁺ + 2e⁻ → H₂ 0.00 V

🔹 Interpretation:

  • Positive E° value: Electrode has a high tendency to get reduced (strong oxidizing agent).
  • Negative E° value: Electrode has a high tendency to get oxidized (strong reducing agent).

🔹 Importance:

  • Helps predict the feasibility of redox reactions
  • Used to construct electrochemical cells
  • Determines cell potential (E°cell) using:

  E°_{\text{cell}} = E°_{\text{cathode}} - E°_{\text{anode}}

Would you like help calculating E°cell or using a standard electrode potential chart?

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