(a) What is the order of a reaction which has a rate constant of 4 × 10−4 mol−2 L
2sec−1 ?
(b) How is the rate of formation of C related to the rate of consumption of B in the reaction given below?
A + 2B → 3C
(c) The rate of a reaction can be expressed as follows:
Rate = k[A][B]3
What will be the rate of the reaction if concentrations of both A and B are doubled?
Answers
Answer:
exp inital [A]
(mol L−1)
inital [B]
(mol L−1)
initial rate of formation of [C]
(mol L−1 sec−1)
1 0.10 0.10 2.5 × 10-4
2 0.20 0.10 5.0 × 10-4
3 0.20 0.50 1.25 × 10-2
1. The initial-rate data in the table above were obtained for
the reaction represented below. What is the experimental
rate law for the reaction.
A + B ⇄ 2 C
a. rate = k[A][B]
b. rate = k[A][B]
2
c. rate = k[A][B]
3
d. rate = k[A]
2
[B]
2
e. rate = k [A]
[B]
2. rate = k[A]2
For the reaction for which rate law is given above, a plot
of which of the following is a straight line?
a.
1
[A]
versus time
b. [A] versus 1
time
c. [A] versus time
d. ln [A] versus time
e. ln [A] versus 1
time
3. 2 X(g) + Y(g) ⇄ 2 Z(g)
When the concentration of substance Y in the reaction
above is doubled, all other factors being held constant, it
is found that the rate of the reaction quadruples. The most
probable explanation for this observation is that
a. substance X is not involved in any of the steps of the
mechanism.
b. substance Y is involved in the rate-determining step
of the mechanism but is not involved in subsequent
steps.
c. substance Y is probably a catalyst and thus speeds up
the rate of the reaction.
d. the reactant with the smallest coefficient in the
balanced equation generally has the greatest effect on
the rate of the reaction.
e. the order of the reaction with respect to Y is 2.
4. The proposed steps for a catalyzed reaction between X4+
and Z+ are represented below.
step 1: X4+ + Y2+ → X3+ + Y3+
step 2: X4+ + Y3+ → X3+ + Y4+
step 3: Y4+ + Z+ → Z3+ + Y2+
The catalyst in this process is
a. X4+
b. X3+
c. Y4+
d. Y2+
e. Z+
5. The balanced equation for the reaction of nitrogen dioxide
and fluorine is
2 NO2 + F2 → 2 NO2F
The proposed mechanism is
step 1: NO2 + F2 → NO2F + F (slow)
step 2: F + NO2 → NO2F (fast)
Which of the following are correct?
I. The mechanism supports an experimentally
determined rate law of rate = k[NO2]2[F2]
II. F is an intermediate
III. The reaction is first order in F2
a. I only
b. I and II only
c. I and III only
d. II and III only
e. I, II, and III
6. Each of the following is true about heterogenous catalyst
EXCEPT
a. Its presence changes the rate of chemical change.
b. It does not undergo a permanent change.
c. It is in the same phase as the reacting particles.
d. It’s presence lowers the activation energy of the
overall reaction.
e. Its presence decreases the potential energy of the
activated complex.
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