• Reaction Quotient (Q)

  • Definition: The ratio of concentration of products to reactants.
  • Kinda like taking a 'snapshot' of where the reaction is at any given moment!

• Chemical Equilibrium

  • Definition: When forward and backward reactions in a reversible reaction occur at the same rate.
  • Symbol: ⇌ (not the usual →).
  • Real-world example: The Haber process to make ammonia. It's like a tug-of-war where both teams are equally strong, so no team can pull the other across the line.

• Equilibrium Constant (K)

  • Definition: The ratio of concentrations of products to reactants when a system is at equilibrium.
  • Fun Fact: It's like the 'destination' for a reversible reaction.

• Q vs. K

  • Comparing these tells us the direction a reaction is moving (forward or backward) towards equilibrium.

• Gibbs Energy (ΔG)

  • Definition: Represents the spontaneity and temperature dependence of a reaction.
  • Rule of Thumb
    • ΔG < 0 ➡️ Reaction is spontaneous (like sliding down a slide! 🎢).
    • ΔG = 0 ➡️ We've hit equilibrium (like pausing at the bottom of the slide! 🛑).
    • ΔG > 0 ➡️ Reaction isn't spontaneous (like trying to climb back up the slide 🧗).

Shape of the Curve & Gibbs Energy

• Region A
  • Here, the forward reaction is partying 🎉! It's favored.
  • Reactants are saying goodbye and products are increasing.
• Equilibrium Point
  • The sweet spot where Q = K.
  • Gibbs energy is at its lowest, just chilling 🍹.
• Region B
  • After the equilibrium point, the forward reaction is tired 😴 (non-spontaneous).
  • ΔG is now positive.
  • The backward reaction takes over the dance floor, becoming spontaneous.