Pearson Baccalaureate Chemistry Higher Level 2nd Edition Print and Online Edition for the IB Diploma
Everything you need to help you with Chemistry chapter 7. These notes are perfectly summarized and organized in subtopic. Includes a compilation of information from the textbook, study guides, class notes and other IB resources. Super easy to read and a great amount of information to help you ace ...
Band 7 SL Chemistry Notes from a 44/45 Novemeber 2022 Graduate
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EQUILIBRIUM
Equilibrium
● System is at equilibrium when rate of forward reaction is equal to the
rate of backward reaction
● Concentrations of reactants + products remain unchanged at
equilibrium
● Reversible reaction = products can reform to produce reactants
● Only occurs in a closed system (only energy but not matter can be
exchanged)
Dynamic equilibrium
● Rate of forward + backward reaction is equal
● No changes at macroscopic level
● Changes in microscopic level
Equilibrium state
1. Dynamic: Reaction hasn't stopped, forwards + backwards reaction
occur at same rate
2. Closed system: No exchange of matter, reactants + products can
recombine
3. Constant concentration of reactants/products: Produced + destroyed
at an equal rate
, 4. No macroscopic changes: Because they depend on concentration of
reactants and products
5. Equilibrium can be reached from either direction
Equilibrium constant (Kc)
● Kc = [Products]^Coefficient stoichiometry/ [Reactants]^Coefficient
stoichiometry
● Kc has a fixed value at a specific temperature
Magnitude of Kc
● Kc > 1 = More products
- [Products] > [Reactants]
● Kc < 1 = More reactants
- [Reactants] > [Products]
● Kc = 1
- [Products] = [Reactants]
- Half-point has been reached
Reaction quotient (Q)
● Q = Equilibrium expression with non-equilibrium concentration of
[Products] and [Reactants]
● Can be used to measure whether reaction is at equilibrium
- Q = Kc → Equilibrium
- Q > Kc → Q decreases as the reaction moves toward equilibrium →
[Reactants] should increase, [Products] should decrease → Reaction
shifts to the left
● Q < Kc → Q increases as the reaction moves towards equilibrium →
[Reactants] should decrease, [Products] should increase → Reaction
shifts to the right
Kc relationships with different reactions
1. Inverse
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