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Equilibrium Constant K quiz #1

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Termini in questo insieme (10)

  • What is the equilibrium constant (K) for pure water at 25°C?
    The equilibrium constant for the autoionization of pure water at 25°C is Kw = 1.0 × 10⁻¹⁴.
  • What does a very small equilibrium constant (K << 1) indicate about a chemical reaction?
    A very small equilibrium constant (K << 1) indicates that the reverse reaction is favored, meaning there are more reactants than products at equilibrium.
  • What is the equilibrium constant expression for the reaction: CO₂(g) + H₂(g) ⇌ CO(g) + H₂O(l)?
    K = [CO] / ([CO₂][H₂]); H₂O(l) is excluded because it is a pure liquid.
  • What is the equilibrium constant expression for the reaction: CO₂(g) + C(s) ⇌ 2 CO(g)?
    K = [CO]² / [CO₂]; C(s) is excluded because it is a solid.
  • What is the value of K for this aqueous reaction at 298 K?
    The value of K at 298 K depends on the specific reaction and its data; it must be calculated using the concentrations of products and reactants at equilibrium.
  • Which K values would indicate that there is more B than A at equilibrium?
    K values greater than 1 indicate that there is more B (product) than A (reactant) at equilibrium.
  • Calculate the value of the equilibrium constant for the reaction.
    To calculate the equilibrium constant, use the equilibrium concentrations of products and reactants in the K expression for the given reaction.
  • What is the equilibrium constant for the reaction above?
    The equilibrium constant for the reaction is determined by substituting the equilibrium concentrations into the appropriate K expression.
  • Estimate the value of the equilibrium constant Kc for the reaction below from the data in the graph.
    To estimate Kc, use the equilibrium concentrations of products and reactants shown in the graph and substitute them into the Kc expression.
  • Write the equilibrium constant expression for this reaction: (aq) + (aq) ⇌ (aq)
    K = [product] / ([reactant₁][reactant₂]); all species are aqueous and included in the expression.