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Equilibrium

Quiz by Natalie Wieland

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23 questions
Show answers
  • Q1
    Which of the following best describes a reaction at equilibrium?
    Reactants are being consumed and products are being formed.
    The concentration of the reactants is equal to the concentration of the products.
    The rate of the forward and reverse reactions are equal.
    The rate of the reaction is zero.
    45s
  • Q2
    What is the equilibrium expression for the given reaction? 2A(aq) + 3B(aq) ⇌ C(aq) + 2D(aq)
    Question Image
    K = ([C][2D])/([2A][3B])
    K = ([A]2[B]3)/([C][D]2)
    K =( [C][D]2)/([A]2[B]3)
    K = ([C] + [D]2)/([A]2 + [B]3)
    60s
  • Q3
    The following boxes represent reactions of the type A <--> B at equilibrium. In which of the following is Keq = 2?
    Question Image
    Reaction III
    All have Keq = 2
    Reaction II
    Reaction I
    60s
  • Q4
    What is the equilibrium constant for the following reaction? 2 KClO3 (s) ⇌ 2 KCl (s) + 3 O2 (g) ΔH < 0
    Question Image
    https://uploads.quizalize.com/7f4b1d9e-cf8d-4c88-b809-1cdb910d2298/question/04a3f7483eefb315c43093848adbe6d8e87cec9c.png
    https://uploads.quizalize.com/7f4b1d9e-cf8d-4c88-b809-1cdb910d2298/question/93ba072f24a4aef1b839f9dfea634265cf6db5eb.png
    Keq = [O2]3
    https://uploads.quizalize.com/7f4b1d9e-cf8d-4c88-b809-1cdb910d2298/question/d2ad90e11cee16b78b5151183f4b8f04831ed766.png
    45s
  • Q5
    Determine the Kc value for the following reaction if the equilibrium concentrations are: [HBr] = 0.20 M, [H2] = 0.10 M, [Br2] = 0.12 M 2 HBr (g) ⇌ H2 (g) + Br2 (g)
    3.33
    6.0 × 10–3
    16.7
    0.30
    120s
  • Q6
    Which of the following statements is FALSE?
    K >> 1 implies that the reaction is very fast at producing products.
    When K >> 1, the forward reaction is favored and essentially goes to completion.
    When K << 1, the reverse reaction is favored and the forward reaction does not proceed to a great extent.
    When K ≈ 1, neither the forward or reverse reaction is strongly favored, and about the same amount of reactants and products exist at equilibrium.
    45s
  • Q7
    Express the equilibrium constant for the following reaction. P4(s) + 5 O2(g) ⇌ P4O10(s)
    K = [P4O10]/([P4][O2]5)
    K = [O2]-5
    K = [O2]5
    K = ([P4][O2]5)/[P4O10]
    45s
  • Q8
    Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [N2]eq = 2.0 M, [H2]eq = 1.0 M, [NH3]eq = 0.50 M. N2(g) + 3 H2(g) ⇌ 2 NH3(g)
    8
    0.125
    2.5
    0.083
    120s
  • Q9
    Once a reaction reaches equilibrium
    the concentration (or pressure) of the reactants and products stop changing
    the concentration (or pressure) of the reactants is greater than that of the products.
    the concentration (or pressure) of the reactants is less than that of the products.
    the concentration (or pressure) of the reactants and products are equal
    30s
  • Q10
    If K<<<<<1 what can you conclude?
    The C(the change in the RICE table) is very small
    The C(the change in the RICE table) is the a ratio based off the limiting reagent
    The C(the change in the RICE table) does not relate to the size of K.
    The C (the change in the RICE table) is very large
    30s
  • Q11
    In the reaction 3W + X < -- > 2Y + Z, all substance are gases. The reaction is initiated by adding an equal number of moles of W and of X. When equilibrium is reached,
    [W] = [X]
    [X] > [W]
    [Y] = [Z]
    [X] = [Y]
    60s
  • Q12
    The reaction 3H2(g) + N2(g) < -- > 2NH3(g), has an enthalpy of change of -92kJ. Increasing the temperature of this equilibrium system causes
    an increase in [NH3]
    a decrease in [H2]
    an increase in [N2]
    an increase in K
    45s
  • Q13
    Consider N2(g) + O2(g) < -- > 2NO (g). The reaction was initiated by adding 15.0 moles of NO to a 1.0L flask. At equilibrium, 3.0 moles of oxygen are present in the 1.0L flask. The value of the K must be
    0.33
    9.0
    5.0
    3.0
    120s
  • Q14
    At a certain temperature, the synthesis of ammonia gas from nitrogen and hydrogen gases, shown as N2(g) + 3H2(g) < -- > 2NH3(g), has a value of K= 0.03. If [H2] = [N2] = 0.10M and [NH3] = 0.20M,
    the reaction would shift toward the N2 and the H2
    the reaction will shift toward a new equilibrium position, but the direction cannot be determined from these data
    the reaction would shift toward the ammonia
    the system is at equilibrium, therefore no shifting will occur
    120s
  • Q15
    One way to produce nitric acid is through the Ostwald process. In the first reaction ammonia is oxidized to nitrogen monoxide, 4NH3(g) + 5O2(g) < -- > 4NO(g) + 6H2O deltaH = -905.2KJ. Which of the following would shift equilibrium to the products?
    lower the temperature of the reaction to condense ammonia into a liquid
    raise the temperature of the reaction and remove nitrogen monoxide as it is made
    raise the temperature of the reaction to keep water in its gaseous form
    Lower the temperature of the reaction and remove nitrogen monoxide as it is made
    60s

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