5 Written questions
5 Matching questions
 Which of the following is a kinetics concept?
a. free energy
b. enthalpy
c. spontaneity
d. reaction mechanism
e. entropy  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. Pseudofirst order
e. Impossible to tell from the given information  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  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  Evaluate the specific rate constant for the reaction at the temperature for which the data were obtained. The ratelaw 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
 a c. 4.0 × 10−1 M−2•min−1
 b b. 0.075 mol/L•min
 c a. Zero order
 d d. reaction mechanism
 e b. 2.01 min−1
5 Multiple choice questions
 d. the reaction of leaded fuels with the catalysts in catalytic converters
 c. 123 kJ
 c. CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
 e. 8.5 min
 b. M−2•s−1
5 True/False questions

Determine the ratelaw 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] 
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 
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 
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 
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