Equilibrium in Chemistry
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Questions and Answers

If the reaction quotient (Q) for a reversible reaction is less than the equilibrium constant (K), which of the following is true?

  • The reaction is at equilibrium.
  • The reaction will not proceed in either direction.
  • The reaction will proceed to the right, favoring products. (correct)
  • The reaction will proceed to the left, favoring reactants.

    • What is the correct expression for the equilibrium constant (K) for the following reaction: 2A + B ⇌ 3C + D?

  • K = [A]^2[B] / [C]^3[D]
  • K = [A][B] / [C][D]
  • K = [C][D] / [A][B]
  • K = [C]^3[D] / [A]^2[B] (correct)

    • Consider the following reversible reaction: A + 2B ⇌ C + D. If the concentration of B is increased, what will be the effect on the equilibrium position?

  • The equilibrium will shift to the right, favoring products. (correct)
  • The equilibrium constant K will decrease.
  • The equilibrium will not be affected.
  • The equilibrium will shift to the left, favoring reactants.

    • Which of the following is an example of a heterogeneous equilibrium?

    <p>CaCO3(s) ⇌ CaO(s) + CO2(g)</p> Signup and view all the answers

    What is the effect of increasing temperature on an endothermic reaction at equilibrium?

    <p>The equilibrium shifts to the right, favoring products.</p> Signup and view all the answers

    Which of the following statements is true about the equilibrium constant (K) for a reversible reaction?

    <p>K can be greater than, less than, or equal to 1.</p> Signup and view all the answers

    What is the effect of increasing pressure on the following equilibrium: N2(g) + 3H2(g) ⇌ 2NH3(g)?

    <p>The equilibrium shifts to the right, favoring products.</p> Signup and view all the answers

    Which of the following factors does NOT affect the position of equilibrium in a reversible reaction?

    <p>Nature of the reactants and products.</p> Signup and view all the answers

    Study Notes

    Equilibrium in Chemistry

    • Definition:

      • A dynamic state where the rate of the forward reaction equals the rate of the reverse reaction.

    • Types of Equilibrium:

      • Chemical Equilibrium: Occurs in reversible chemical reactions.
      • Physical Equilibrium: Involves physical changes, like phase transitions (e.g., solid-liquid).

    • Characteristics:

      • Concentrations of reactants and products remain constant over time.
      • The system can be disturbed, leading to shifts in concentrations.

    • Le Chatelier's Principle:

      • If a system at equilibrium is disturbed, it will adjust to minimize the disturbance.
      • Changes that can shift equilibrium:
        • Concentration changes
        • Temperature changes
        • Pressure changes (for gases)

    • Equilibrium Constant (K):

      • A ratio of the concentrations of products to reactants, each raised to the power of their coefficients.
      • For a reaction: aA + bB ⇌ cC + dD:
        • K = [C]^c [D]^d / [A]^a [B]^b
      • Values of K indicate:
        • K > 1: favors products
        • K < 1: favors reactants

    • Homogeneous vs. Heterogeneous Equilibrium:

      • Homogeneous: All reactants and products are in the same phase.
      • Heterogeneous: Reactants and products are in different phases; solids and liquids are not included in the equilibrium expression.

    • Reaction Quotient (Q):

      • Similar to K, but for non-equilibrium conditions.
      • Q = [products]^coefficients / [reactants]^coefficients
      • Comparison of Q and K determines the direction of the shift:
        • Q < K: shifts right (toward products)
        • Q > K: shifts left (toward reactants)

    • Factors Affecting Equilibrium:

      • Concentration: Adding/removing reactants/products shifts the equilibrium.
      • Temperature:
        • Endothermic reactions: Increase in temperature shifts right.
        • Exothermic reactions: Increase in temperature shifts left.
      • Pressure:
        • Increasing pressure shifts equilibrium toward the side with fewer moles of gas.

    • Applications:

      • Used in industrial processes (e.g., Haber process for ammonia synthesis).
      • Important in biological systems (e.g., enzyme activity, respiration).

    Equilibrium in Chemistry

    • Dynamic Equilibrium:

      • Occurs when the rates of forward and reverse reactions are equal.

    • Types of Equilibrium:

      • Chemical Equilibrium: Involves reversible reactions where products can revert to reactants.
      • Physical Equilibrium: Pertains to physical changes such as phase transitions (e.g., solid to liquid).

    • Equilibrium Characteristics:

      • Constant concentrations of reactants and products over time.
      • Systems can be disturbed, resulting in shifts in concentrations.

    • Le Chatelier's Principle:

      • If disturbed, an equilibrium system will shift to counter the effect of the disturbance.
      • Disturbances include changes in concentration, temperature, or pressure (for gases).

    • Equilibrium Constant (K):

      • Represents the ratio of product concentrations to reactant concentrations, elevated to their coefficients.
      • For reaction: aA + bB ⇌ cC + dD, K is calculated as:
        • K = [C]^c [D]^d / [A]^a [B]^b.
      • Interpretation of K values:
        • K > 1 indicates a favoring of products.
        • K < 1 indicates a favoring of reactants.

    • Homogeneous vs. Heterogeneous Equilibrium:

      • Homogeneous Equilibrium: All species are in the same phase (gas, liquid, etc.).
      • Heterogeneous Equilibrium: Different phases are present; solids and liquids are omitted from equilibrium expressions.

    • Reaction Quotient (Q):

      • Similar concept to K but applicable during non-equilibrium conditions.
      • Q = [products]^coefficients / [reactants]^coefficients.
      • Comparison provides insight into the shift direction:
        • Q < K indicates a shift to the right (towards products).
        • Q > K indicates a shift to the left (towards reactants).

    • Factors Influencing Equilibrium:

      • Concentration: Adding or removing substances causes shifts in equilibrium.
      • Temperature:
        • In endothermic reactions, an increase in temperature shifts equilibrium towards products.
        • In exothermic reactions, an increase shifts it towards reactants.
      • Pressure:
        • Increasing pressure favors the side of the reaction with fewer moles of gas.

    • Applications of Equilibrium:

      • Crucial in industrial chemistry, such as ammonia production via the Haber process.
      • Significant in biological contexts, influencing processes like enzyme activity and cellular respiration.

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    Description

    Explore the concept of equilibrium in chemistry, focusing on the dynamic state where the rate of the forward reaction equals the rate of the reverse reaction. This quiz covers types of equilibrium, including chemical and physical, as well as their characteristics and importance in chemical reactions.

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