Equilibrium – Interactive Quiz & Cheatsheet

Master chemical and ionic equilibrium concepts with this interactive quiz and reference guide

Updated: just now

Categories: Mini Game, Chemistry, Class 11, Physical Chemistry
Tags: Mini Game, Chemistry, Class 11, Equilibrium, Chemical Equilibrium, Ionic Equilibrium, Le Chatelier's Principle
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Equilibrium Cheatsheet & Quiz

Equilibrium Cheatsheet

Cheat Codes & Shortcuts

  • Chemical Equilibrium: State where forward and reverse reaction rates are equal.
  • Dynamic Nature: Both reactions continue at equal rates; no net change.
  • Equilibrium Constant (\(K_c\)): \(K_c = \frac{[Products]}{[Reactants]}\) at equilibrium.
  • Le Chatelier’s Principle: System shifts to oppose changes in concentration, pressure, temperature.
  • Reaction Quotient (\(Q\)): Same form as \(K\), but for non-equilibrium.
  • Relationship: \(Q < K\) forward favoured; \(Q > K\) reverse favoured.
  • Effect of Temperature: Endothermic reaction: increase shifts right, exothermic: shifts left.
  • Effect of Pressure: Increasing pressure favours side with fewer moles gas.
  • Homogeneous Equilibrium: Equilibrium species in same phase.
  • Heterogeneous Equilibrium: Different phases; solids/liquids omitted in \(K_c\) expression.

Quick Reference Table

Term Definition / Formula Example / Note
Equilibrium Constant, \(K_c\) \(K_c = \frac{[C]^c [D]^d}{[A]^a [B]^b}\) for \(\mathrm{aA + bB \rightleftharpoons cC + dD}\) Only gases and aqueous species included
Reaction Quotient, \(Q\) Calculated same as \(K_c\), but at any point Compare with \(K_c\) to predict direction
Le Chatelier's Principle System shifts to counteract disturbance Add reactant → shift right
Effect of Pressure Increased pressure favors side with fewer moles gas \( \mathrm{N_2 + 3H_2 \rightleftharpoons 2NH_3} \) - Pressure increase shifts right
Effect of Temperature Endothermic favor forward on heating; exothermic favor reverse Heat added shifts equilibrium
Heterogeneous Equilibrium Phases differ; solids/liquids omit from \(K_c\) \( \mathrm{CaCO_3(s) \rightleftharpoons CaO(s) + CO_2(g)} \)

Advice

Step 1: Write balanced chemical equation and expression for \(K_c\).

Step 2: Calculate or use given initial concentrations to find \(Q\).

Step 3: Compare \(Q\) and \(K_c\) to predict reaction direction.

Step 4: Apply Le Chatelier’s principle for changes in concentration, pressure, temperature.

Step 5: For heterogeneous equilibria, omit pure solids/liquids in expressions.

Equilibrium Quick Tips

  • Calculate \(K_c\): Concentrations raised to stoichiometric powers.
  • Reaction Quotient \(Q\): Use initial concentrations to decide direction.
  • Temperature effects: Consider endothermic/exothermic nature carefully.
  • Pressure effects: Count moles of gases on each side.
  • Solid and liquid phases: Not included in equilibrium expressions.

Equilibrium Speed Quiz

Test your speed with 5 equilibrium questions! You have 30 seconds per question.