Kinetics ❮ 205- The energy difference between the reactants and
the transition state is:
(A) the free energy
(B) the heat of reaction
(C) the activation energy
(D) the kinetic energy - Which of the following is the reason it is neces-
sary to strike a match against the side of a box to
light the match?
(A) It is necessary to supply the free energy for
the reaction.
(B) It is necessary to supply the activation energy
for the reaction.
(C) It is necessary to supply the heat of reaction
for an endothermic reaction.
(D) It is necessary to supply the heat of reaction
for an exothermic reaction. - The following table gives the initial concentra-
tions and rate for three experiments.
EXPERIMENT
INITIAL
[CO]
(mol L-^1 )INITIAL
[Cl 2 ]
(mol L-^1 )INITIAL RATE OF
FORMATION
OF COCL 2 (mol L-^1
min-^1 )
1 0.200 0.100 3.9 × 10 -^25
2 0.100 0.200 3.9 × 10 -^25
3 0.200 0.200 7.8 × 10-^25The reaction is CO(g) + Cl 2 (g) → COCl 2 (g).
What is the rate law for this reaction?
(A) Rate = k[CO]
(B) Rate = k[CO]^2 [Cl 2 ]
(C) Rate = k[CO][Cl 2 ]
(D) Rate = k[CO][Cl 2 ]^2
- The reaction (CH 3 ) 3 CBr(aq) + H 2 O(l) →
(CH 3 ) 3 COH(aq) + HBr(aq) follows the rate law
Rate = k[(CH 3 ) 3 CBr]. What will be the effect of
decreasing the concentration of (CH 3 ) 3 CBr?
(A) The rate of the reaction will increase.
(B) More HBr will form.
(C) The rate of the reaction will decrease.
(D) The reaction will shift to the left.
11. When the concentration of H+(aq) is doubled for
the reaction H 2 O 2 (aq) + 2 Fe^2 +(aq) + 2 H+(aq) →
2 Fe^3 +(aq) + 2 H 2 O(g), there is no change in the
reaction rate. This indicates that:
(A) the H+ is a spectator ion
(B) the rate-determining step does not involve H+
(C) the reaction mechanism does not involve H+
(D) the H+ is a catalyst
12. The following mechanism has been proposed for
the reaction of CHCl 3 with Cl 2 :
Step l Cl 2 (g) → 2 Cl(g) fast
Step 2 Cl(g) + CHCl (g) → CCl 3 (g) + 3 HCl(g) slow
Step 3 CCl 3 (g) + Cl(g) → CCl 4 (g) fastWhich of the following rate laws is consistent
with this mechanism?
(A) Rate = k[Cl 2 ]
(B) Rate = k[CHCl 3 ] [Cl 2 ]
(C) Rate = k[CHCl 3 ]
(D) Rate = k[CHCl 3 ] [Cl 2 ]1/2- The reaction NO 2 (g) + CO(g) → NO(g) + CO 2 (g)
has the rate law Rate = k[NO 2 ]^2. In one experi-
ment, the initial amounts of NO 2 and CO were
both 0.100 M. In another experiment, the initial
concentration of CO was doubled to 0.200 M,
and the concentration of NO 2 remained the
same (0.100 M). All other variables remained
unchanged. Which of the following expresses how
the rate of the second experiment compares to
that of the first experiment?
(A) The rate of both experiments is the same.
(B) The rate of the second experiment is double
the first.
(C) The rate of the second experiment is one-half
the first.
(D) There is insufficient information to make a
conclusion.