Chapter 14 Barbara Mowery York College The rate of a reaction can be increased by increasing reactant concentrations increasing the temperature adding a suitable catalyst d All of the ID: 426660
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Slide1
Clicker QuestionsChapter 14
Barbara Mowery
York CollegeSlide2
The rate of a reaction can be increased byincreasing reactant concentrations.increasing the temperature.
adding a suitable catalyst.d. All of the
aboveSlide3
The rate of a reaction can be increased byincreasing reactant concentrations.increasing the temperature.
adding a suitable catalyst.d. All of the
aboveSlide4
Over time, the rate of most chemical reactions tends to _______.increasedecrease
remain constantd. oscillateSlide5
Over time, the rate of most chemical reactions tends to _______.increasedecrease
remain constantd. oscillateSlide6
Consider the reaction A2 + 3 B2 3 AB3
. If ΔA is
–0.750
M/min, then
Δ
B is
–0.750 M/min.
–0.225
M/min.
–0.250
M/min.
2.25
M/min.Slide7
Consider the reaction A2 + 3 B2 3 AB3
. If ΔA is –0.750
M/min, then
Δ
B is
–0.750
M/min.
–0.225
M/min.
–0.250
M/min.
2.25
M/min.Slide8
If tripling the concentration of reactant A multiplies the rate by a factor of nine, the reaction is _______ order in A.zerothfirst
secondd. thirdSlide9
If tripling the concentration of reactant A multiplies the rate by a factor of nine, the reaction is _______ order in A.zerothfirst
secondd. thirdSlide10
The relationship that allows us to study changes in concentration by measuring the absorption of light is Rate = k[A][B].
A = εbc.
ln
[A]
t
=
–
kt
+
ln
[A]
0
.
t
½
=
0.693/k.Slide11
The relationship that allows us to study changes in concentration by measuring the absorption of light is Rate = k[A][B].
A = εbc.
ln
[A]
t
=
–
kt
+
ln
[A]
0
.
t
½
=
0.693/k.Slide12
Select the incorrect statement.The exponents in a rate law are taken from the coefficients in the balanced reaction.
For a first-order reaction, the plot of ln[A] versus time is linear.For a zero-order reaction, the plot of [A] versus time is a parabola.
The slope of 1/[A] versus time is the half-life of a first-order reaction.Slide13
Select the incorrect statement.The exponents in a rate law are taken from the coefficients in the balanced reaction.
For a first-order reaction, the plot of ln[A] versus time is linear.For a zero-order reaction, the plot of [A] versus time is a parabola.The slope of 1/[A] versus time is the half-life of a first-order reaction.Slide14
Reaction: A + B C + DRate = k[A][B]The overall order of this reaction is
first.second.
third.
d. fourth.Slide15
Reaction: A + B C + DRate = k[A][B]The overall order of this reaction is
first.second.
third.
d. fourth.Slide16
Reaction: W + X Y + ZRate = k[W]
The order of this reaction with respect to X iszeroth.
first.
second.
d. third.Slide17
Reaction: W + X Y + ZRate = k[W]
The order of this reaction with respect to X iszeroth.
first.
second.
d. third.Slide18
The time required for the concentration of a reactant to be reduced to half of its initial value is called themidpoint of the reaction.equivalence point of the reaction.
half-rate of the reaction.d. half-life of the reaction.Slide19
The time required for the concentration of a reactant to be reduced to half of its initial value is called themidpoint of the reaction.equivalence point of the reaction.
half-rate of the reaction.d. half-life of the reaction.Slide20
If k is the rate constant of a first-order reaction, the half-life of the reaction is0.693/k.
0.693k.k/2.
d.
2k.Slide21
If k is the rate constant of a first-order reaction, the half-life of the reaction is0.693/k.
0.693k.k/2.
d.
2k.Slide22
The value of the rate constant (k) for a first-order reaction is 0.010 sec–1. What is the half-life of this reaction?
10 seconds69 seconds100 seconds
d. 690 secondsSlide23
The value of the rate constant (k) for a first-order reaction is 0.010 sec–1. What is the half-life of this reaction?
10 seconds69 seconds100 seconds
d. 690 secondsSlide24
A + B products, Rate = k[A],k = 0.010 sec–1
, Initial [A] = .100 M, Final [A] = .00100 M How long will this take?
69 seconds
138 seconds
460 seconds
d. 690 secondsSlide25
A + B products, Rate = k[A],k = 0.010 sec–1
, Initial [A] = .100 M, Final [A] = .00100 M How long will this take?
69 seconds
138 seconds
460 seconds
d. 690 secondsSlide26
Rate = k[A]2, Initial [A] = 0.100 M, k = 0.0214 M–1 sec–1 What is the half-life of this second-order reaction?
69 seconds138 seconds
460 seconds
d. 690 secondsSlide27
Rate = k[A]2, Initial [A] = 0.100 M, k = 0.0214 M–1 sec–1 What is the half-life of this second-order reaction?
69 seconds138 seconds
460 seconds
d. 690 secondsSlide28
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?0.0500 M
0.0250 M
0.0189 M
d. 0.0115 MSlide29
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?0.0500 M
0.0250 M
0.0189 M
d. 0.0115 MSlide30
The minimum energy that a collision between molecules must have for a reaction to occur is called theinitial energy.internal energy.
external energy.d. energy of activation.Slide31
The minimum energy that a collision between molecules must have for a reaction to occur is called theinitial energy.internal energy.
external energy.d. energy of activation.Slide32
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
100 kJ/mole.
310 kJ/mole.
690 kJ/mole.
d. 1000 kJ/mole.Slide33
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
100 kJ/mole.
310 kJ/mole.
690 kJ/mole.
d. 1000 kJ/mole.Slide34
The rate-determining step is the _______ step in a reaction mechanism.firstlast
c. fastestd. slowestSlide35
The rate-determining step is the _______ step in a reaction mechanism.firstlast
c. fastestd. slowestSlide36
In a reaction mechanism, a species that is produced in an early step and consumed in a later step is called ___.a byproducta catalyst
an intermediatea reactantSlide37
In a reaction mechanism, a species that is produced in an early step and consumed in a later step is called ___.a byproducta catalyst
an intermediatea reactantSlide38
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 byproducta catalyst
an intermediatea reactantSlide39
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 byproducta catalyst
an intermediatea reactantSlide40
Adding a catalyst increases the rate of a chemical reaction because the presence of the catalystincreases molecular velocities.increases molecular collisions.
decreases energy of activation.d. All of the aboveSlide41
Adding a catalyst increases the rate of a chemical reaction because the presence of the catalystincreases molecular velocities.increases molecular collisions.
decreases energy of activation.d. All of the above