Chapter 13 – Rates of Reaction
1. Nitric oxide reacts with hydrogen at a measurable rate at 1000 K according to the following
equation:
2NO + 2H2 → N2 + 2H2O
The experimental rate law is Rate = k[NO]2[H2]. If time is measured in minutes and
concentration is measured in moles per liter, what are the units for the rate of production of
water?
A)
L2/(mol2 · min).
B)
mol2/(L2 · min).
C)
mol/(L · min).
D)
mol3/(L3 · min).
E)
mol/(L2 · min).
2. Which of the following conclusions concerning the concentration-time plot provided below
is/are correct?
1.
The concentration of substance D is decreasing over time.
2.
The instantaneous reaction rate at point A is less than the instantaneous
reaction rate at point B.
3.
Substance D is a product of the reaction.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
1, 2, and 3
3. Which of the following is/are expected to affect the rate of a chemical reaction?
1.
Increasing the reaction temperature.
2.
Decreasing the reactant concentrations.
3.
Doubling the volume of the reaction container.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
1, 2, and 3
4. The oxidation of ammonia produces nitrogen and water via the following reaction:
4NH3(g) + 3O2(g) → 2N2(g) + 6H2O(l)
Suppose the rate of formation of H2O(l) is 3.0 mol/(L · s). Which of the following
statements is true?
A)
The rate of consumption of NH3 is 2.0 mol/(L · s).
B)
The rate of consumption of O2 is 2.0 mol/(L · s).
C)
The rate of formation of N2 is 1.3 mol/(L · s).
D)
The rate of formation of N2 is 2.0 mol/(L · s).
E)
The rate of consumption of NH3 is 0.50 mol/(L · s).
5. For the reaction
IO3–(aq) + 5I–(aq) + 6H+(aq) → 3I2(aq) + 3H2O(l)
the rate of disappearance of I–(aq) at a particular time and concentration is 2.6 10–
3 mol/(L · s). What is the rate of appearance of I2(aq)?
A)
4.3 10–3 mol/(L · s)
B)
7.8 10–3 mol/(L · s)
C)
–1.6 10–3 mol/(L · s)
D)
1.6 10–3 mol/(L · s)
E)
6.4 10–3 mol/(L · s)
Test Bank General Chemistry, 10th edition 3
6. For the reaction
6CH2O(aq) + 4NH3(aq) → (CH2)6N4(aq) + 6H2O(l)
the rate of the reaction may be expressed as . What is an equivalent expression
for the rate of the reaction?
A)
B)
C)
D)
E)
7. For the hypothetical reaction A + 2B → 2C + D, the initial rate of disappearance of A is
2.0 10–2 mol/(L · s). What is the initial rate of disappearance of B?
A)
8.0 10–2 mol/(L · s)
B)
4.0 10–2 mol/(L · s)
C)
1.4 10–1 mol/(L · s)
D)
4.0 10–4 mol/(L · s)
E)
1.4 10–2 mol/(L · s)
KEY: change of concentration with time MSC: general chemistry
8. For the reaction
2N2O5(g) → 4NO2(g) + O2(g)
which of the following expressions is equal to the rate of the reaction?
A)
B)
C)
Test Bank General Chemistry, 10th edition 4
D)
E)
9. For the reaction of the ammonium ion with nitrous acid, the net reaction is
NH4+(aq) + HNO2(aq) → N2(g) + 2H2O(l) + H+(aq)
If the initial concentration of nitrous acid is 1.00 M and, after 28.8 s has elapsed, the
concentration of nitrous acid has fallen to 0.82 M, what is the average rate of the reaction
over this time interval?
A)
0.0063 M/s
B)
0.028 M/s
C)
–0.0063 M/s
D)
–0.028 M/s
E)
0.063 M/s
10. In the reaction 2H2O2(aq) → 2H2O(l) + O2(g), the initial concentration of H2O2 is 0.542 M
and, 21.2 seconds later, the concentration of H2O2 is 0.310 M. What is the average rate of
reaction over this time interval?
A)
–0.0109 M/s
B)
0.0109 M/s
C)
0.0146 M/s
D)
0.00547 M/s
E)
–0.00547 M/s
11. Which of the following experimental methods cannot be used to measure the rate of a
reaction?
A)
measurement of the absorbance of a colored reactant with time
B)
measurement of the change in the partial pressure of a gas-phase product over time
C)
measurement of the equilibrium concentration of an acidic product via titration
with a strong base
D)
measurement of the absorbance of a colored product with time
E)
measurement of the change in the partial pressure of a gas-phase reactant over time
Test Bank General Chemistry, 10th edition 5
12. Which of the following statements concerning the experimental determination of reaction
rates is incorrect?
A)
To determine reaction rates one of the reactants must be colored.
B)
Monitoring changes in reactant or product physical properties is a convenient way
to determine reaction rates.
C)
Analysis of samples withdrawn from the reaction solution at varying times is
useful for slow reactions.
D)
Instrumental methods, such as visible spectroscopy, may be used to continuously
measure changes in reactants or products.
E)
Any method of analysis that can determine product or reactant concentrations
during the course of the reaction can potentially be used to determine reaction
rates.
13. Which of the following statements is true concerning the reaction given below?
2H2S(g) + O2(g) → 2S(s) + 2H2O(g)
A)
The rate law is Rate = k[H2S]2[O2].
B)
The reaction is second-order in H2S(g) and first-order in O2(g).
C)
The reaction is first-order in H2S(g) and second-order in O2(g).
D)
The rate law is Rate = k[H2S][O2].
E)
The rate law may be determined only by experiment.
14. Consider the reaction
aA + bB dD + eE C = catalyst
The rate law is
Rate = k[A]q[B]r[C]s
Which of the following statements is incorrect?
A)
The exponents q and r are always equal to the coefficients a and b, respectively.
B)
The overall reaction order is q + r + s.
C)
The exponent s must be determined experimentally.
D)
The symbol k represents the rate constant.
E)
The exponents q, r, and s are often integers.
15. For a second-order reaction, what are the possible units of the rate constant?
A)
L–1 · s–1
B)
mol · L–1 · s–1
C)
s
D)
L.mol–1s–1
E)
mol · L–1
16. For which of the following hypothetical rate laws would the units of the rate constant have
the general form M−time−?
A)
rate = k[A]3
B)
rate = k[A]4
C)
rate = k[A]2
D)
rate = k[A]
E)
rate = k
17. If the rate law for a reaction is
Rate = k[ClO3–][I–][H+]2
what are the units of k when the unit of time is seconds and the unit of concentration is
moles per liter?
A)
(L · s)/mol
B)
mol2/(L2 · s)
C)
mol/(L · s)
D)
L2/(mol2 · s)
E)
L3/(mol3 · s)
Test Bank General Chemistry, 10th edition 7
18. The hypochlorite ion oxidizes the iodide ion in aqueous solution as represented by the
following equation:
OCl–(aq) + I–(aq) → OI–(aq) + Cl–(aq)
The rate law for this reaction is Rate = k. If time is measured in seconds and
concentration is measured in moles per liter, what are the units for k?
A)
mol2/(L2 · s)
B)
L/(mol · s)
C)
1/s
D)
L2/(mol2 · s)
E)
mol/(L · s)
19. For a certain first-order reaction with the general form aA → products, the rate is 0.32 M·s−
when the concentration of the reactant is 0.29 M. What is the rate constant for this reaction?
A)
0.26 s−
B)
1.1 s−
C)
0.32 s−
D)
3.1 s−
E)
3.8 s−
20. Which of the following statements is always true?
A)
Exothermic reactions have lower activation energies than endothermic reactions.
B)
The rate of a catalyzed reaction is independent of the concentration of the catalyst.
C)
The rate for a reaction depends on the concentrations of all the reactants.
D)
The rate constant is independent of the concentrations of the reacting species.
E)
The rate law can be determined from the stoichiometric equation.
21. Which of the following statements is incorrect?
A)
The rates of most chemical reactions change with time.
B)
The rate constant for a reaction can be changed by changing the temperature.
C)
The rate constant is dependent on the reactant concentrations.
D)
In a series of stepwise reactions, the rate-determining step is the slowest one.
E)
The rate of a catalyzed reaction is dependent on the concentration of the catalyst.
22. A rate constant for a particular reaction is 0.0070 M-1s−. What is the overall order of this
reaction?
A)
2
B)
3
C)
4
D)
0
E)
1
23. Ozone reacts with nitrogen dioxide to produce oxygen and dinitrogen pentoxide according
to the following chemical equation:
O3(g) + 2NO2(g) → O2(g) + N2O5(g)
The rate law for this reaction is Rate = k[O3][NO2]. If concentration is measured in moles
per liter and time is measured in seconds, what are the units of k?
A)
L · mol–1 · s
B)
L2 · mol–2 · s–1
C)
L · mol–1 · s–1
D)
mol · L–1 · s–1
E)
mol2 · L–2 · s–1
24. The balanced chemical equation and rate law for the reaction between NO(g) and H2(g) at a
particular temperature are
2NO(g) + 2H2(g) → N2(g) + 2H2O(g)
Rate = k[NO]2[H2]
What is the reaction order with respect to hydrogen?
A)
4
B)
0
C)
2
D)
3
E)
1
25. The reaction
2H2(g) + 2NO(g) → 2H2O(g) + N2(g)
is first-order in H2 and second-order in NO at a particular temperature. What is the rate law?
A)
Rate = k[H2]2[NO]2
B)
Rate = k[H2][NO]2
C)
Rate = k[H2][NO]
D)
Rate = k[H2O]2[N2]
E)
Rate = k[H2]2[NO]
26. The hypochlorite ion oxidizes the iodide ion in aqueous solution as represented by the
following equation:
OCl–(aq) + I–(aq) → OI–(aq) + Cl–(aq)
The rate law for this reaction is Rate = k. The overall reaction order and the
order with respect to OH– are
A)
2 and –1.
B)
0 and –1.
C)
0 and 1.
D)
2 and 1.
E)
1 and –1.
27. The rate law for the chemical reaction
5Br–(aq) + BrO3–(aq) + 6H+(aq) → 3Br2(aq) + 3H2O(l)
has been determined experimentally to be Rate = k[Br–][BrO3–][H+]2. What is the overall
order of the reaction?
A)
3
B)
5
C)
4
D)
2
E)
1
28. If a reaction is first-order with respect to a particular reactant, when the concentration of that
reactant is increased by a factor of 2, the reaction rate will _____.
A)
increase by a factor of 2.
B)
remain constant.
C)
decrease by a factor of
1
2
.
D)
decrease by a factor of
1
8
.
E)
increase by a factor of 4.
29. The following data were obtained for the hypothetical reaction 2A + B → products.
[A]0 (M)
[B]0 (M)
Initial Rate (M/s)
0.2
0.1
5
0.2
0.2
20
0.6
0.1
45
What is the overall order of this reaction?
A)
3
B)
1/2
C)
0
D)
4
E)
1
30. For the reaction between nitrogen monoxide and chlorine to produce nitrosyl chloride,
2NO(g) + Cl2(g) → 2NOCl(g), it is found that tripling the initial concentration of both
reactants increases the initial rate by a factor of 27. If only the initial concentration of
chlorine is tripled, the initial rate increases by a factor of 3. What is the order of the reaction
with respect to Cl2?
A)
1/2
B)
1
C)
2
D)
3
E)
0
Test Bank General Chemistry, 10th edition 11
31. For the reaction
(CH3)3CCl(aq) + OH–(aq) → (CH3)3COH(aq) + Cl–(aq)
it is found experimentally that doubling the initial concentration of (CH3)3CCl causes the
initial reaction rate to double, but doubling the initial concentration of OH– has no effect on
the rate. What is the rate law?
A)
Rate = k[(CH3)3CCl]2[OH–]
B)
Rate = k[(CH3)3CCl][OH–]
C)
Rate = k
D)
Rate = k[(CH3)3COH][Cl–]
E)
Rate = k[(CH3)3CCl]
32. If a reaction is zero-order in a reactant, when the concentration of the reactant is decreased
by a factor of 2, the reaction rate will
A)
quadruple.
B)
decrease by a factor of 1/2.
C)
remain constant.
D)
decrease by a factor of 1/4.
E)
double.
KEY: dependence of rate on concentration | reaction order MSC: general chemistry
33. The following data were obtained in a kinetics study of the hypothetical reaction A + B + C
→ products.
[A]0 (M)
[B]0 (M)
[C]0 (M)
Initial Rate (10–3 M/s)
0.4
0.4
0.2
160
0.2
0.4
0.4
80
0.6
0.1
0.2
15
0.2
0.1
0.2
5
0.2
0.2
0.4
20
Using the initial-rate method, what is the order of the reaction with respect to A?
A)
first-order
B)
zero-order
C)
third-order
D)
second-order
E)
impossible to tell from the data given
34. Nitrosyl chloride is produced from the reaction of nitrogen monoxide and chlorine:
2NO(g) + Cl2(g) → 2NOCl(g)
The following initial rates at a given temperature were obtained for the concentrations listed
below.
Experiment
Initial Rate (mol·L–1·h–1)
[NO]0 (mol·L–1)
[Cl2]0 (mol·L–1)
1
2.21
0.25
0.25
2
19.89
0.75
0.25
3
6.63
0.25
0.75
From the data, what is the experimental rate law?
A)
Rate = k[Cl2]
B)
Rate = k[NO]
C)
Rate = k[NO][Cl2]2
D)
Rate = k[NO]2[Cl2]
E)
Rate = k[NO][Cl2]1/2
35. For the reaction A + B + C → products, the following initial-rate data were obtained.
[A]0 (mol/L)
[B]0 (mol/L)
[C]0 (mol/L)
Initial Rate (mol/(L · s))
0.40
0.40
0.20
0.0160
0.20
0.40
0.40
0.0080
0.60
0.10
0.20
0.0015
0.20
0.10
0.20
0.0005
0.20
0.20
0.40
0.0020
What are the reaction orders with respect to A, B, and C, respectively?
A)
0, 1, 1
B)
1, 2, 1
C)
1, 1, 1
D)
1, 2, 0
E)
0, 2, 1
Test Bank General Chemistry, 10th edition 13
36. The acid-catalyzed reaction of acetone, CH3COCH3, with iodine can be represented by the
following net reaction:
CH3COCH3 + I2 CH2ICOCH3 + H+ + I–
It is found experimentally that the rate law for this reaction is Rate = k[CH3COCH3][H+].
Suppose that in trial 1, the initial rate of the reaction is measured with the initial
concentrations of acetone, iodine, and hydrogen ion all equal to 0.10 M. Then, in trial 2, the
initial rate of the reaction is measured with the initial concentrations all equal to 0.20 M.
The initial rate of trial 2 will be larger than the initial rate of trial 1 by a factor of
A)
4.
B)
16.
C)
8.
D)
2.
E)
64.
37. The rate law for the hydrolysis of thioacetamide (CH3CSNH2),
CH3CSNH2(aq) + H2O(l) → H2S(g) + CH3CONH2(aq)
is Rate = k[H+][CH3CSNH2]. If, during the course of the reaction, some solid sodium
hydroxide is added to the reaction mixture, then
A)
the reaction rate decreases, but k remains the same.
B)
the reaction rate remains the same, but k decreases.
C)
the reaction rate increases, but k remains the same.
D)
there is no change in the reaction rate or the rate constant.
E)
the reaction rate remains the same, but k increases.
38. The rate law for the reaction between chlorine and nitric oxide,
2NO(g) + Cl2(g) → 2NOCl(g)
is Rate = k[NO]2[Cl2]. Which of the following changes will not alter the initial rate of the
reaction?
A)
increasing the concentration of NOCl
B)
decreasing the volume of the reaction system
C)
running the reaction in a solvent rather than in the gas phase
D)
increasing the volume of the reaction system
E)
increasing the concentration of chlorine gas
39. In aqueous solution, iodine reacts with acetone as represented by the following equation:
I2(aq) + CH3COCH3(aq) → CH3COCH2I(aq) + H+(aq) + I–(aq)
The experimental rate law is Rate = k[H+][CH3COCH3]. According to the information
above, an increase in the hydrogen ion concentration has what effect on the reaction?
A)
It decreases the rate of the reaction.
B)
It increases the rate of the reaction.
C)
It decreases the value of the equilibrium constant.
D)
It increases the value of the equilibrium constant.
E)
It does not affect the rate of the reaction.
40. The reaction between selenous acid and the iodide ion in acid solution is
H2SeO3(aq) + 6I–(aq) + 4H+(aq) → Se(s) + 2I3–(aq) + 3H2O(l)
The data in the following table were measured at 0°C.
Experiment
[H2SeO3]0 (M)
[H+]0 (M)
[I–]0 (M)
Initial Rate [mol/(L · s)]
1
1.00 10–4
2.00 10–2
3.00 10–2
5.30 10–7
2
2.00 10–4
2.00 10–2
3.00 10–2
1.06 10–6
3
3.00 10–4
4.00 10–2
3.00 10–2
6.36 10–6
4
3.00 10–4
8.00 10–2
3.00 10–2
2.54 10–5
5
3.00 10–4
8.00 10–2
6.00 10–2
2.04 10–4
6
2.00 10–4
2.00 10–2
6.00 10–2
8.48 10–6
The overall order of this reaction is
A)
4.
B)
6.
C)
2.
D)
8.
E)
3.
41. The reaction between selenous acid and the iodide ion in acid solution is
H2SeO3(aq) + 6I–(aq) + 4H+(aq) → Se(s) + 2I3–(aq) + 3H2O(l)
The data in the following table were measured at 0°C.
Experiment
[H2SeO3]0 (M)
[H+]0 (M)
[I–]0 (M)
Initial Rate [mol/(L · s)]
1
1.00 10–4
2.00 10–2
3.00 10–2
5.30 10–7
2
2.00 10–4
2.00 10–2
3.00 10–2
1.06 10–6
3
3.00 10–4
4.00 10–2
3.00 10–2
6.36 10–6
4
3.00 10–4
8.00 10–2
3.00 10–2
2.54 10–5
5
3.00 10–4
8.00 10–2
6.00 10–2
2.04 10–4
6
2.00 10–4
2.00 10–2
6.00 10–2
8.48 10–6
What is the rate constant for this reaction?
A)
1.5 104 L5/(mol5 · s)
B)
1.5 1010 L5/(mol5 · s)
C)
4.9 105 L5/(mol5 · s)
D)
294 L5/(mol5 · s)
E)
8.8 L5/(mol5 · s)
42. Two substances A and B react with each other in such a way that one-half of A remains
after 25 min and one-fourth of A remains after 50 min. Doubling the concentration of B
while keeping the concentration of A fixed doubles the rate of the reaction. This reaction is
A)
first-order in both A and B.
B)
zero-order in both A and B.
C)
second-order in A and first-order in B.
D)
first-order in A and second-order in B.
E)
second-order in both A and B.
Test Bank General Chemistry, 10th edition 16
43. The reaction between selenous acid and the iodide ion in acid solution is
H2SeO3(aq) + 6I–(aq) + 4H+(aq) → Se(s) + 2I3–(aq) + 3H2O(l)
The data in the following table were measured at 0°C.
Experiment
[H2SeO3]0 (M)
[H+]0 (M)
[I–]0 (M)
Initial Rate [mol/(L · s)]
1
1.00 10–4
2.00 10–2
3.00 10–2
5.30 10–7
2
2.00 10–4
2.00 10–2
3.00 10–2
1.06 10–6
3
3.00 10–4
4.00 10–2
3.00 10–2
6.36 10–6
4
3.00 10–4
8.00 10–2
3.00 10–2
2.54 10–5
5
3.00 10–4
8.00 10–2
6.00 10–2
2.04 10–4
6
2.00 10–4
2.00 10–2
6.00 10–2
8.48 10–6
Tripling the initial concentration of H2SeO3 while holding the initial concentrations of H+
and I– constant increases the rate of the reaction by a factor of
A)
8.
B)
4.
C)
3.
D)
2.
E)
1.
44. The reaction between selenous acid and the iodide ion in acid solution is
H2SeO3(aq) + 6I–(aq) + 4H+(aq) → Se(s) + 2I3–(aq) + 3H2O(l)
The data in the following table were measured at 0°C.
Experiment
[H2SeO3]0 (M)
[H+]0 (M)
[I–]0 (M)
Initial Rate [mol/(L · s)]
1
1.00 10–4
2.00 10–2
3.00 10–2
5.30 10–7
2
2.00 10–4
2.00 10–2
3.00 10–2
1.06 10–6
3
3.00 10–4
4.00 10–2
3.00 10–2
6.36 10–6
4
3.00 10–4
8.00 10–2
3.00 10–2
2.54 10–5
5
3.00 10–4
8.00 10–2
6.00 10–2
2.04 10–4
6
2.00 10–4
2.00 10–2
6.00 10–2
8.48 10–6
Tripling the initial concentration of H+ while holding the initial concentrations of H2SeO3
and I– constant increases the initial rate of the reaction by a factor of
A)
9.
B)
16.
C)
32.
D)
2.
E)
4.
Test Bank General Chemistry, 10th edition 17
45. The reaction between selenous acid and the iodide ion in acid solution is
H2SeO3(aq) + 6I–(aq) + 4H+(aq) → Se(s) + 2I3–(aq) + 3H2O(l)
The data in the following table were measured at 0°C.
Experiment
[H2SeO3]0 (M)
[H+]0 (M)
[I–]0 (M)
Initial Rate [mol/(L · s)]
1
1.00 10–4
2.00 10–2
3.00 10–2
5.30 10–7
2
2.00 10–4
2.00 10–2
3.00 10–2
1.06 10–6
3
3.00 10–4
4.00 10–2
3.00 10–2
6.36 10–6
4
3.00 10–4
8.00 10–2
3.00 10–2
2.54 10–5
5
3.00 10–4
8.00 10–2
6.00 10–2
2.04 10–4
6
2.00 10–4
2.00 10–2
6.00 10–2
8.48 10–6
Tripling the initial concentration of I– while holding the initial concentrations of H2SeO3 and
H+ constant increases the initial rate of the reaction by a factor of
A)
27.
B)
9.
C)
3.
D)
8.
E)
6.
46. Which of the following corresponds to the correct integrated expression for a second-order
reaction?
A)
B)
C)
D)
E)
47. Which of the following is not a correct representation of the integrated rate expression for a
first-order reaction?
A)
B)
C)
D)
E)
48. At a given temperature, a first-order reaction has a rate constant of 3.5 10–3 s–1. How long
will it take for the reaction to be 24% complete?
A)
410 s
B)
1200 s
C)
910 s
D)
34 s
E)
78 s
49. A chemical reaction that is first-order in X is observed to have a rate constant of 2.20 10–2
s–1. If the initial concentration of X is 1.0 M, what is the concentration of X after 186 s?
A)
0.20 M
B)
0.017 M
C)
64 M
D)
0.59 M
E)
0.98 M
50. The nuclide 96Nb decays by a first-order process with a rate constant of 2.96 10–2 h–1. How
long will it take for 82.0% of the initial amount of 96Nb to be consumed?
A)
33.8 h
B)
57.9 h
C)
27.7 h
D)
6.70 h
E)
6.08 h
51. The radioactive nuclide 63Ni decays by a first-order process via the emission of a beta
particle. The 63Ni nuclide has a half-life of 100. years. How long will it take for 71% of 63Ni
to decay?
A)
49.4 years
B)
21.5 years
C)
0.858 years
D)
179 years
E)
77.6 years
52. The gas-phase decomposition of N2O5 is a first-order process with a rate constant of
1.50 10–3 s–1 at 55°C. The decomposition reaction is
N2O5(g) → 2NO2(g) + O2(g)
If 2.0 g of N2O5 is placed in vessel 1 and 1.0 g of N2O5 in vessel 2 and the vessels are at the
same temperature (55°C) and the same pressure, how much time is required for half of the
N2O5 to decompose in each vessel?
A)
Vessel 1 requires the same amount of time as vessel 2.
B)
Vessel 1 requires twice as much time as vessel 2.
C)
Vessel 1 requires three times as much time as vessel 2.
D)
Vessel 1 requires four times as much time as vessel 2.
E)
Vessel 2 requires twice as much time as vessel 1.
Test Bank General Chemistry, 10th edition 20
53. A reaction that is second-order in one reactant has a rate constant of 2.2 10–2 L/(mol · s). If
the initial concentration of the reactant is 0.360 mol/L, how long will it take for the
concentration to become 0.180 mol/L?
A)
320 s
B)
63 s
C)
1300 s
D)
32 s
E)
130 s
54. The nuclide 188W decays by a first-order process with a rate constant of 1.0 10–2 d–1. How
long will it take for 91% of the initial amount of 188W to be consumed?
A)
4.1 d
B)
220 d
C)
9.4 d
D)
240 d
E)
110 d
55. For the hypothetical first-order reaction A → products, k = 0.0839 s–1. If the initial
concentration of A is 0.640 M, how long would it take for A to be 66.4% consumed?
A)
8.26 s
B)
13.0 s
C)
11.9 s
D)
18.6 s
E)
4.88 s
56. For the hypothetical second-order reaction A → products, k = 0.319 M–1 s–1. If the initial
concentration of A is 0.834 M, how long would it take for A to be 94.8% consumed?
A)
0.206 s
B)
3.76 s
C)
9.27 s
D)
68.5 s
E)
0.167 s