Think you’ve got your head wrapped around Kinetics? Put your knowledge to
the test. Good luck — the Stickman is counting on you!
Q. What are the units of reaction rate?
L mol-1 s-1
L2 mol-2 s-1
s-1
mol L-1 s-1
None of the above
Q. For the following chemical equation, which of the following is correct? 2H2S + O2 → 2S + 2H2O
The reaction is third-order overall.
The reaction is second-order overall.
The rate law is rate = k[H2S]2[O2].
The rate law cannot be determined from the given information.
The rate law is rate = k[H2S][O2].
Q. The reaction A + B → C has a reaction rate which is experimentally observed to follow rate = k[A]2[B]. If the concentration of A is tripled and the concentration of B is doubled, the reaction rate would be increased by a factor of _______.
6
9
12
18
None of the Above
Q. The reaction of A + 2B → C was found to have rate = k[A][B]2. While holding the concentration of A constant, the concentration of B was increased from 1x to 3x. By what factor will the rate of the reaction increase?
2
3
9
27
None of the above
Q. For A + 3B → 2C the rate should be expressed as _______.
rate = d[A]/dt
rate = -d[C]/dt
rate = -3d[B]/dt
rate = d[C]/2dt
None of the above
Q. The reaction A + 2B → C has a rate law of rate = k[A][B]3. When the concentration of B is doubled, while A is unchanged, by what factor will the rate of the reaction increase?
2
4
6
8
None of the Above
Q. The reaction A + 2B → C has a rate law of rate = k[A][B]2. By what factor does the rate of the reaction increase when the concentration of A is doubled and the concentration of B is also doubled?
2
4
6
8
None of the above
Q. The reaction A + 2B → C has a rate law of rate = k[A] 2[B]. By what factor does the rate of the reaction increase when the concentration of A is doubled and the concentration of B is tripled?
5
6
12
18
None of the Above
Q. What are the units for a first-order rate constant?
M/s
1/Ms-1
1/s
1/M2s
None of the above
Q. When a catalyst is added to a system at equilibrium, a decrease occurs in the _______.
activation energy
heat of reaction
potential energy of the reactants
potential energy of the products
None of the above