7.1 Introduction to Equilibrium

• What is chemical equilibrium in reversible reactions?

  Equal forward and reverse rates
• Dynamic equilibrium is a state where the forward reaction rate equals the reverse reaction rate
• How does increasing the concentration of reactants affect equilibrium?

  Shifts equilibrium forward
• For the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g), what happens to equilibrium if pressure is increased?

  Equilibrium shifts forward
• What is dynamic equilibrium in a reversible process?

  Forward rate equals reverse rate
• How does increasing the concentration of a reactant affect equilibrium?

  Shifts equilibrium forward
• What is the key difference between reversible and irreversible reactions in terms of direction?

  Reversible reactions go both ways
• What conditions favor ammonia production in the Haber-Bosch process?

  High pressure, moderate temperature
• What ions are formed when a weak acid dissolves in water?

  H₃O⁺ and A⁻
• At chemical equilibrium, the forward and reverse reactions occur at equal rates.


  True
• What is the difference between dynamic and static equilibrium?

  Dynamic has ongoing reactions
• Increasing pressure in a reaction shifts the equilibrium toward the side with fewer moles of gas
• What are the three key properties of chemical equilibrium?

  Reversible reactions, equal rates, constant concentrations
• Static equilibrium involves no change or movement at all.


  True
• For exothermic reactions, increasing temperature shifts the equilibrium backward.
• Match the equilibrium system with its description:

  Haber-Bosch Process ↔️ Combines nitrogen and hydrogen to produce ammonia

  Dissolution of Weak Acids ↔️ Forms hydrogen ions and conjugate bases
• The equilibrium constant for the dissolution of weak acids is typically low.
• What happens to the concentrations of reactants and products at equilibrium?

  They remain constant
• In dynamic equilibrium, the system is in a steady state with continuous forward and reverse reactions.

  True
• For an exothermic reaction, increasing temperature shifts the equilibrium backward.


  True
• At equilibrium, the concentrations of reactants and products must be equal.

  False
• Changes in concentration, pressure, and temperature can affect the equilibrium of a reversible reaction by shifting it to favor the forward or reverse reaction.
• Irreversible reactions are denoted by the double arrow symbol (⇌).

  False
• The Haber-Bosch process uses the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g).


  True