Study Guide: Reaction Rates, Equilibrium and Acids & Bases

Study Guide: Reaction Rates, Equilibrium and Acids & Bases

Study Guide: Reaction Rates and Equilibrium

Holt Chemistry: Chapters 16 and 14

  1. The rate of a reaction is measured by the amount of (reactants/products) formed over time.
  2. In order for a reaction to occur, the reactant molecules must have enough (concentration/time/energy).
  3. Will the following increase or decrease the rate of a reaction?
    A. grinding up a piece of zinc
    B. adding an inhibitor
    C. decreasing the temperature
    D. adding a catalyst
    E. using a large chunk of iron in a reaction instead of smaller pieces
    F. decreasing the concentration of a reactant
  4. To react, particles must (collide/have the same energy/have different energies/all of the above).
  5. Draw the energy diagram for an exothermic AND endothermic reaction. Label: reactant, product, activated complex, activation energy and heat (ΔH). Include in both diagrams the pathway a catalyst would take.
  6. Define activation energy.
  7. How does a catalyst affect activation energy?
  8. What is an activated complex?
  9. Define equilibrium.Draw the arrow
  10. What does Le Chatelier’s Principle State?
  11. Problem: Using the following equation, predict the equilibrium shift (left or right) if the following stresses are added: 2 SO2 (g) + O2 (g) ⇋ 2 SO3 (g) + heat
    a. O2 is added to the reaction.
    b. SO2 is added to the reaction.
    c. SO3 is added to the reaction.
    d. The pressure is increased.
    e. The temperature was decreased.
  12. Write the equilibrium constant expression for the equation in #11.
  13. If in the equilibrium reaction listed in #11 the concentration of SO2 is 0.034 M, O2 is 0.003M and SO3 is 1.2M, what is the equilibrium constant?
  14. Which phase of matter will be affected when the pressure of an equilibrium reaction is increased? (solid/liquid/gas/aqueous)
  15. NH4Cl(s) + heat  NH3(g) + HCl(g)
    What kind of change will shift the reaction above the right to form more products?
    A. a decrease in total pressure
    B. an increase in the concentration of HCl
    C. an increase in the pressure of NH3
    D. a decrease in temperature
  16. H2 + Cl2→2 HCl
    Which of the these describes the rate of this chemical reaction?
    A. an increase in the concentration of HCl and H2 with time
    B. an increase in the concentration of HCl with time
    C. an increase in H2 and Cl2 with time
    D. a decrease in HCl and Cl2with time
  17. C6H6 + Br2→C6H5Br + HBr
    Which of the following changes will cause an increase in the rate of the above reaction?
    A. increasing the concentration of Br2
    B. decreasing the concentration of C6H6
    C. increasing the concentration of HBr
    D. decreasing the temperature
  18. In which of the following reactions involving gases would the forward reaction (shift to the right) be favored by an increase in pressure?
    A. A + B  AB
    B. A + B  C + D
    C. 2 A + B  C + 2 D
    D. AC  A + C
  19. 4 HCl(g) + O2(g) 2 H2O(l) + 2 Cl2(g) + 113 kJ
    Which action will drive the reaction to the right?
    A. heating the equilibrium mixture
    B. adding water to the system
    C. decreasing the oxygen concentration
    D. increasing the system’s pressure
  20. Using the equations below, answer the questions.

A + B → C(fast)Step 1

C → D + E(slow)Step 2

E + F → G + H(fast)Step 3

  1. Which of the 3 steps (1, 2 or 3) is the rate-determining step?
  2. Would the addition of substance C increase the rate of reaction?
  3. Would the addition of substance E increase the rate of reaction?