Clicker Questions
Chapter 14
Barbara Mowery
York College
© 2015 Pearson Education, Inc.
The rate of a reaction can be
increased by
a.
b.
c.
d.
increasing reactant concentrations.
increasing the temperature.
adding a suitable catalyst.
All of the above
© 2015 Pearson Education, Inc.
The rate of a reaction can be
increased by
a.
b.
c.
d.
increasing reactant concentrations.
increasing the temperature.
adding a suitable catalyst.
All of the above
© 2015 Pearson Education, Inc.
Over time, the rate of most
chemical reactions tends to
_______.
a.
b.
c.
d.
increase
decrease
remain constant
oscillate
© 2015 Pearson Education, Inc.
Over time, the rate of most
chemical reactions tends to
_______.
a.
b.
c.
d.
increase
decrease
remain constant
oscillate
© 2015 Pearson Education, Inc.
Consider the reaction
A2 + 3 B2 3 AB3. If ΔA is
–0.750 M/min, then ΔB is
a.
b.
c.
d.
–0.750 M/min.
–0.225 M/min.
–0.250 M/min.
2.25 M/min.
© 2015 Pearson Education, Inc.
Consider the reaction
A2 + 3 B2 3 AB3. If ΔA is
–0.750 M/min, then ΔB is
a.
b.
c.
d.
–0.750 M/min.
–0.225 M/min.
–0.250 M/min.
2.25 M/min.
© 2015 Pearson Education, Inc.
If tripling the concentration of
reactant A multiplies the rate
by a factor of nine, the reaction
is _______ order in A.
a.
b.
c.
d.
zeroth
first
second
third
© 2015 Pearson Education, Inc.
If tripling the concentration of
reactant A multiplies the rate
by a factor of nine, the reaction
is _______ order in A.
a.
b.
c.
d.
zeroth
first
second
third
© 2015 Pearson Education, Inc.
The relationship that allows us
to study changes in
concentration by measuring
the absorption of light is
a.
b.
c.
d.
Rate = k[A][B].
A = εbc.
ln[A] t = –kt + ln[A]0.
t ½ = 0.693/k.
© 2015 Pearson Education, Inc.
The relationship that allows us
to study changes in
concentration by measuring
the absorption of light is
a.
b.
c.
d.
Rate = k[A][B].
A = εbc.
ln[A] t = –kt + ln[A]0.
t ½ = 0.693/k.
© 2015 Pearson Education, Inc.
Select the incorrect statement.
a. The exponents in a rate law are
taken from the coefficients in the
balanced reaction.
b. For a first-order reaction, the plot of
ln[A] versus time is linear.
c. For a zero-order reaction, the plot
of [A] versus time is a parabola.
d. The slope of 1/[A] versus time is the
half-life of a first-order reaction.
© 2015 Pearson Education, Inc.
Select the incorrect statement.
a. The exponents in a rate law are
taken from the coefficients in the
balanced reaction.
b. For a first-order reaction, the plot of
ln[A] versus time is linear.
c. For a zero-order reaction, the plot
of [A] versus time is a parabola.
d. The slope of 1/[A] versus time is the
half-life of a first-order reaction.
© 2015 Pearson Education, Inc.
Reaction: A + B  C + D
Rate = k[A][B]
The overall order of this
reaction is
a.
b.
c.
d.
first.
second.
third.
fourth.
© 2015 Pearson Education, Inc.
Reaction: A + B  C + D
Rate = k[A][B]
The overall order of this
reaction is
a.
b.
c.
d.
first.
second.
third.
fourth.
© 2015 Pearson Education, Inc.
Reaction: W + X  Y + Z
Rate = k[W]
The order of this reaction with
respect to X is
a.
b.
c.
d.
zeroth.
first.
second.
third.
© 2015 Pearson Education, Inc.
Reaction: W + X  Y + Z
Rate = k[W]
The order of this reaction with
respect to X is
a.
b.
c.
d.
zeroth.
first.
second.
third.
© 2015 Pearson Education, Inc.
The time required for the
concentration of a reactant to
be reduced to half of its initial
value is called the
a.
b.
c.
d.
midpoint of the reaction.
equivalence point of the reaction.
half-rate of the reaction.
half-life of the reaction.
© 2015 Pearson Education, Inc.
The time required for the
concentration of a reactant to
be reduced to half of its initial
value is called the
a.
b.
c.
d.
midpoint of the reaction.
equivalence point of the reaction.
half-rate of the reaction.
half-life of the reaction.
© 2015 Pearson Education, Inc.
If k is the rate constant of a
first-order reaction, the half-life
of the reaction is
a.
b.
c.
d.
0.693/k.
0.693k.
k/2.
2k.
© 2015 Pearson Education, Inc.
If k is the rate constant of a
first-order reaction, the half-life
of the reaction is
a.
b.
c.
d.
0.693/k.
0.693k.
k/2.
2k.
© 2015 Pearson Education, Inc.
The value of the rate constant
(k) for a first-order reaction is
0.010 sec–1. What is the halflife of this reaction?
a.
b.
c.
d.
10 seconds
69 seconds
100 seconds
690 seconds
© 2015 Pearson Education, Inc.
The value of the rate constant
(k) for a first-order reaction is
0.010 sec–1. What is the halflife of this reaction?
a.
b.
c.
d.
10 seconds
69 seconds
100 seconds
690 seconds
© 2015 Pearson Education, Inc.
A + B  products, Rate = k[A],
k = 0.010 sec–1, Initial [A] =
.100 M, Final [A] = .00100 M
How long will this take?
a.
b.
c.
d.
69 seconds
138 seconds
460 seconds
690 seconds
© 2015 Pearson Education, Inc.
A + B  products, Rate = k[A],
k = 0.010 sec–1, Initial [A] =
.100 M, Final [A] = .00100 M
How long will this take?
a.
b.
c.
d.
69 seconds
138 seconds
460 seconds
690 seconds
© 2015 Pearson Education, Inc.
Rate = k[A]2, Initial [A] = 0.100 M,
k = 0.0214 M–1 sec–1
What is the half-life of this secondorder reaction?
a.
b.
c.
d.
69 seconds
138 seconds
460 seconds
690 seconds
© 2015 Pearson Education, Inc.
Rate = k[A]2, Initial [A] = 0.100 M,
k = 0.0214 M–1 sec–1
What is the half-life of this secondorder reaction?
a.
b.
c.
d.
69 seconds
138 seconds
460 seconds
690 seconds
© 2015 Pearson Education, Inc.
Rate = k[A]2, Initial [A] =
0.100 M, k = 0.0214 M–1 sec–1
After 1.00 hour, what is the
concentration of reactant A?
a.
b.
c.
d.
0.0500 M
0.0250 M
0.0189 M
0.0115 M
© 2015 Pearson Education, Inc.
Rate = k[A]2, Initial [A] =
0.100 M, k = 0.0214 M–1 sec–1
After 1.00 hour, what is the
concentration of reactant A?
a.
b.
c.
d.
0.0500 M
0.0250 M
0.0189 M
0.0115 M
© 2015 Pearson Education, Inc.
The minimum energy that a
collision between molecules
must have for a reaction to
occur is called the
a.
b.
c.
d.
initial energy.
internal energy.
external energy.
energy of activation.
© 2015 Pearson Education, Inc.
The minimum energy that a
collision between molecules
must have for a reaction to
occur is called the
a.
b.
c.
d.
initial energy.
internal energy.
external energy.
energy of activation.
© 2015 Pearson Education, Inc.
At 298 K, k = 1.36  10–7 sec–1.
At 323 K, k = 2.72  10–6 sec–1.
The energy of activation for this
reaction is
a.
b.
c.
d.
100 kJ/mole.
310 kJ/mole.
690 kJ/mole.
1000 kJ/mole.
© 2015 Pearson Education, Inc.
At 298 K, k = 1.36  10–7 sec–1.
At 323 K, k = 2.72  10–6 sec–1.
The energy of activation for this
reaction is
a.
b.
c.
d.
100 kJ/mole.
310 kJ/mole.
690 kJ/mole.
1000 kJ/mole.
© 2015 Pearson Education, Inc.
The rate-determining step is
the _______ step in a reaction
mechanism.
a.
b.
c.
d.
first
last
fastest
slowest
© 2015 Pearson Education, Inc.
The rate-determining step is
the _______ step in a reaction
mechanism.
a.
b.
c.
d.
first
last
fastest
slowest
© 2015 Pearson Education, Inc.
In a reaction mechanism, a
species that is produced in an
early step and consumed in a
later step is called ___.
a.
b.
c.
d.
a byproduct
a catalyst
an intermediate
a reactant
© 2015 Pearson Education, Inc.
In a reaction mechanism, a
species that is produced in an
early step and consumed in a
later step is called ___.
a.
b.
c.
d.
a byproduct
a catalyst
an intermediate
a reactant
© 2015 Pearson Education, Inc.
In a reaction mechanism, a
species on the reactant side
initially that is consumed in an
early step and regenerated in
a later step is called ___.
a.
b.
c.
d.
a byproduct
a catalyst
an intermediate
a reactant
© 2015 Pearson Education, Inc.
In a reaction mechanism, a
species on the reactant side
initially that is consumed in an
early step and regenerated in
a later step is called ___.
a.
b.
c.
d.
a byproduct
a catalyst
an intermediate
a reactant
© 2015 Pearson Education, Inc.
Adding a catalyst increases
the rate of a chemical reaction
because the presence of the
catalyst
a.
b.
c.
d.
increases molecular velocities.
increases molecular collisions.
decreases energy of activation.
All of the above
© 2015 Pearson Education, Inc.
Adding a catalyst increases
the rate of a chemical reaction
because the presence of the
catalyst
a.
b.
c.
d.
increases molecular velocities.
increases molecular collisions.
decreases energy of activation.
All of the above
© 2015 Pearson Education, Inc.