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5 Written questions

5 Matching questions

  1. Which of the following is a kinetics concept?
    a. free energy
    b. enthalpy
    c. spontaneity
    d. reaction mechanism
    e. entropy
  2. For a certain reaction, a plot of reactant concentration as a function of time gave a straight line. What is the order of this reaction?
    a. Zero order
    b. First order
    c. Second order
    d. Pseudo-first order
    e. Impossible to tell from the given information
  3. Consider the following first order reaction.
    A2B → AB + A

    If it takes 87 seconds for the concentration of A2B to be reduced from 2.2 M to 0.12 M, what is the value of the specific rate constant?
    a. 0.0334 min−1
    b. 2.01 min−1
    c. 2.01 s−1
    d. 18.3 min−1
    e. 3.51 × 10−3 s−1
  4. In the following reaction, the rate of formation of NH3 is 0.15 mol/L•min. What is the rate of reaction?
    N2 + 3H2 → 2NH3

    a. 0.15 mol/L•min
    b. 0.075 mol/L•min
    c. −0.075 mol/L•min
    d. 0.20 mol/L•min
    e. 0.30 mol/L•min
  5. Evaluate the specific rate constant for the reaction at the temperature for which the data were obtained. The rate-law expression is rate = k[A][B]2.
    A + B → C

    Experiment Initial [A] Initial [B] Initial Rate of Formation of C
    1 0.10 M 0.10 M 4.0 × 10−4 M/min
    2 0.20 M 0.20 M 3.2 × 10−3 M/min
    3 0.10 M 0.20 M 1.6 × 10−3 M/min

    a. 1.2 × 10−2 M−2•min−1
    b. 3.6 × 10−2 M−2•min−1
    c. 4.0 × 10−1 M−2•min−1
    d. 6.2 × 10−1 M−2•min−1
    e. 7.0 × 10−3 M−2•min−1
  1. a c. 4.0 × 10−1 M−2•min−1
  2. b b. 0.075 mol/L•min
  3. c a. Zero order
  4. d d. reaction mechanism
  5. e b. 2.01 min−1

5 Multiple choice questions

  1. d. the reaction of leaded fuels with the catalysts in catalytic converters
  2. c. 123 kJ
  3. c. CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
  4. e. 8.5 min
  5. b. M−2•s−1

5 True/False questions

  1. Determine the rate-law expression for the reaction below:
    2A + B2 + C → Α2B + BC

    Trial Initial [A] Initial [B2] Initial [C] Initial Rate of Formation of BC
    1 0.20 M 0.20 M 0.20 M 2.4 × 10−6 M•min−1
    2 0.40 M 0.30 M 0.20 M 9.6 × 10−6 M•min−1
    3 0.20 M 0.30 M 0.20 M 2.4 × 10−6 M•min−1
    4 0.20 M 0.40 M 0.40 M 4.8 × 10−6 M•min−1

    a. rate = k[A]2[B2][C]
    b. rate = k[B2]2[C]2
    c. rate = k[A][C]2
    d. rate = k[A]2[C]
    e. rate = k[A][B2][C]
    d. rate = k[A]2[C]

          

  2. Which of the following statements regarding temperature and reaction rate is false.
    a. The Arrhenius equation can be used to find the activation energy of a reaction.
    b. Reaction rate always increases with higher temperature.
    c. A larger negative value of ΔG0 causes a faster reaction rate.
    d. A larger value of Ea causes a slower reaction rate.
    e. The rate constant for a reaction decreases at lower temperatures.
    c. A larger negative value of ΔG0 causes a faster reaction rate

          

  3. The second order reaction below has a rate constant of 5.76 M−1•min−1 at 1600 K.
    2CH4 → C2H2 + 3H2

    How long would it take for the concentration of CH4 to be reduced from 0.89 M to 5.25 × 10−4 M?
    a. 165 hrs
    b. 0.15 hrs
    c. 2.75 hrs
    d. 5.51 hrs
    e. 9.27 hrs
    c. 2.75 hrs

          

  4. The reaction below has the following rate law: rate = 0.011 L/mol•s [SF4]2.
    SF4 → SF2 + F2

    How many minutes will it take for the concentration of SF4 to be reduced from 2.5 M to 0.25 M?
    a. 327 min
    b. 0.025 min
    c. 5.5 min
    d. 0.040 min
    e. 22.7 min
    c. 5.5 min

          

  5. Which of the following is/are expected to affect the rate of a chemical reaction?
    1. Increasing the reaction temperature.
    2. Addition of a catalyst.
    3. Stirring a well mixed reaction solution.



    a. 1 only
    b. 2 only
    c. 3 only
    d. 1 and 2
    e. 1, 2, and 3
    d. 1 and 2

          

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