111111 chemistry 132 nt more can be accomplished with the phrase “i must do something” than with...
TRANSCRIPT
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111111
Chemistry 132 NT
More can be accomplished with the phrase “I must do something” than with the phrase “something should be done”.
Anon
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222222
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Rates of Reaction
Chapter 13
Module 2
Section 13.4
The burning of steel wool
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444444
Review
The effect of concentration on reaction rate.
Determination of the Rate Law for a given reaction by the method of initial rates.
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555555
Change of Concentration with Time
A rate law simply tells you how the rate of reaction changes as reactant concentrations change.
A more useful mathematical relationship would show how a reactant concentration changes over a period of time.
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666666
Change of Concentration with Time
A rate law simply tells you how the rate of reaction changes as reactant concentrations change.
Using calculus we can transform a rate law into a mathematical relationship between concentration and time.
This provides a graphical method for determining rate laws.
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777777
Concentration-Time Equations
Zero-Order Rate Law
Suppose we look at a simple generic zero order reaction of the reactant “A” to form products.
products A Remember that the rate of this reaction is unaffected by the concentration of “A”.
kk[A]Rate o It’s Rate Law would be:
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888888
Concentration-Time Equations
Zero-Order Rate Law
You could write the rate law in the form;
k]A[k t
]A[ Rate o
Using calculus, we can derive the following relationship between [A] and time,”t”.
ot ]A[kt]A[
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999999
Concentration-Time Equations
Zero-Order Rate Law
You could write the rate law in the form;
k]A[k t
]A[ Rate o
Here [A]t is the concentration of reactant A
at time t, and [A]o is the initial concentration.
ot ]A[kt]A[
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101010101010
A Problem To Consider
Suppose that the decomposition of a hypothetical compound “A” is zero order with a rate constant of 1.8 x 10-4 (mol/L.s). If the initial concentration of “A” is 1.00 mol/L, what is the concentration of “A” after 600 seconds?
The zero-order concentration-time equation for this reaction would be:
ot ]A[kt]A[
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111111111111
A Problem To Consider
Suppose that the decomposition of a hypothetical compound “A” is zero order with a rate constant of 1.8 x 10-4 (mol/L.s). If the initial concentration of “A” is 1.00 mol/L, what is the concentration of “A” after 600 seconds?
L/mol )]00.1()600)(108.1([]A[ 4t
Substituting the given information we obtain:
L/mol )]00.1()108.0([]A[ t
L/mol 892.0]A[ t
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121212121212
Concentration-Time Equations
First-Order Rate Law
Suppose we look at a simple generic first order reaction of the reactant “A” to form products.
products A In a first-order reaction, the rate is directly proportional to the concentration of “A”.
k[A]Rate Its Rate Law would be:
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131313131313
Concentration-Time Equations
First-Order Rate Law
You could write the rate law in the form;
]A[k t
]A[ Rate
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141414141414
Concentration-Time Equations
First-Order Rate Law
Using calculus, you get the following equation.
kt- ]A[]A[
lno
t
Here [A]t is the concentration of reactant A at time t, and [A]o is the initial concentration.
The ratio [A]t/[A]o is the fraction of A remaining at time t.
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151515151515
A Problem To Consider
The decomposition of N2O5 to NO2 and O2 is first order with a rate constant of 4.8 x 10-4 s-1. If the initial concentration of N2O5 is 1.65 x 10-2 mol/L, what is the concentration of N2O5 after 825 seconds?The first-order time-concentration equation for this reaction would be:
kt- ]ON[]ON[
lno52
t52
?
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161616161616
A Problem To Consider
The decomposition of N2O5 to NO2 and O2 is first order with a rate constant of 4.8 x 10-4 s-1. If the initial concentration of N2O5 is 1.65 x 10-2 mol/L, what is the concentration of N2O5 after 825 seconds?Substituting the given information we obtain:
s) 825()s10(4.80- L/mol1065.1
]ON[ln 1-4-
2t52
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171717171717
A Problem To Consider
The decomposition of N2O5 to NO2 and O2 is first order with a rate constant of 4.8 x 10-4 s-1. If the initial concentration of N2O5 is 1.65 x 10-2 mol/L, what is the concentration of N2O5 after 825 seconds?Substituting the given information we obtain:
0.396- L/mol1065.1
]ON[ln 2
t52
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181818181818
A Problem To Consider
The decomposition of N2O5 to NO2 and O2 is first order with a rate constant of 4.8 x 10-4 s-1. If the initial concentration of N2O5 is 1.65 x 10-2 mol/L, what is the concentration of N2O5 after 825 seconds?Taking the inverse natural log of both sides we obtain:
673.0 L/mol1065.1
]ON[ 0.396-2
t52 e
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191919191919
A Problem To Consider
The decomposition of N2O5 to NO2 and O2 is first order with a rate constant of 4.8 x 10-4 s-1. If the initial concentration of N2O5 is 1.65 x 10-2 mol/L, what is the concentration of N2O5 after 825 seconds?Solving for [N2O5] at 825 s we obtain:
L/mol 0111.0)673.0()L/mol101.65(]O[N 2-52
(see Exercise 13.5 and Problem 13.49)
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202020202020
A Problem To Consider
In the presence of excess thiocyanate ion, SCN-, the following reaction is first order in iron(III) ion, Fe3+; the rate constant, k, is 1.27 h-1.
How many hours are required for this reaction to reach 90% completion?
(aq)Fe(SCN)(aq)SCN (aq)Fe 2-3
First, we must note that a 90% completion implies that only 10% of the reactants are left. This implies
10.0][Fe
][Fe
o3
t3
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212121212121
A Problem To Consider
In the presence of excess thiocyanate ion, SCN-, the following reaction is first order in iron(III) ion, Fe3+; the rate constant, k, is 1.27 h-1.
How many hours are required for this reaction to reach 90% completion?
(aq)Fe(SCN)(aq)SCN (aq)Fe 2-3
Going to our first-order concentration-time equation, we obtain:
kt][Fe
][Feln
o3
t3
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222222222222
A Problem To Consider
In the presence of excess thiocyanate ion, SCN-, the following reaction is first order in iron(III) ion, Fe3+; the rate constant, k, is 1.27 h-1.
How many hours are required for this reaction to reach 90% completion?
(aq)Fe(SCN)(aq)SCN (aq)Fe 2-3
Substituting values for k and the ratio [Fe3+]t/Fe3+]o
t)h 27.1()10.0ln( 1-
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232323232323
A Problem To Consider
In the presence of excess thiocyanate ion, SCN-, the following reaction is first order in iron(III) ion, Fe3+; the rate constant, k, is 1.27 h-1.
How many hours are required for this reaction to reach 90% completion?
(aq)Fe(SCN)(aq)SCN (aq)Fe 2-3
Solving for t we get:
hours 81.1h 27.1
ln(0.10)t 1-
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242424242424
Concentration-Time Equations
Second-Order Rate Law
You could write the rate law in the form
2]A[k t
]A[ Rate
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252525252525
Concentration-Time Equations
Second-Order Rate Law
Using calculus, you get the following equation.
ot [A]1
kt ]A[
1
Here [A]t is the concentration of reactant A at time t, and [A]o is the initial concentration.
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262626262626
Concentration-Time Equations
Rate Law SummaryThe following table summarizes the Rate Laws and concentration-time equations we have just outlined.
Rate Law Concentration-time equation
Zero-order Rate=k[A]0
First-order Rate = k[A]1
Second-order Rate = k[A]2
ot ]A[kt]A[
kt- lno
t
]A[]A[
ot [A]1
]A[1 kt
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272727272727
Half-life
The half-life of a reaction is the time required for the reactant concentration to decrease to one-half of its initial value.
For a first-order reaction, the half-life is independent of the initial concentration of reactant.
21kt)ln(2
1
In one half-life the amount of reactant decreases by one-half. Substituting into the first-order concentration-time equation, we get:
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282828282828
Half-life
The half-life of a reaction is the time required for the reactant concentration to decrease to one-half of its initial value.
Solving for t1/2 we obtain:
k693.0
t21
Figure 13.8 illustrates the half-life of a first-order reaction.
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Figure 13.8
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303030303030
Half-life
Sulfuryl chloride, SO2Cl2, decomposes in a first-order reaction to SO2 and Cl2.
At 320 oC, the rate constant is 2.2 x 10-5 s-1. What is the half-life of SO2Cl2 vapor at this temperature?
)g(Cl)g(SO)g(ClSO 2222
Substitute the value of k into the relationship between k and t1/2.
k693.0
t21
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313131313131
Half-life
Sulfuryl chloride, SO2Cl2, decomposes in a first-order reaction to SO2 and Cl2.
At 320 oC, the rate constant is 2.2 x 10-5 s-1. What is the half-life of SO2Cl2 vapor at this temperature?
)g(Cl)g(SO)g(ClSO 2222
Substitute the value of k into the relationship between k and t1/2.
1-5 s 1020.2
693.0t
21
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323232323232
Half-life
Sulfuryl chloride, SO2Cl2, decomposes in a first-order reaction to SO2 and Cl2.
At 320 oC, the rate constant is 2.2 x 10-5 s-1. What is the half-life of SO2Cl2 vapor at this temperature?
)g(Cl)g(SO)g(ClSO 2222
Substitute the value of k into the relationship between k and t1/2.
s1015.3t 421
(see Exercise 13.6 and Problem 13.53)
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333333333333
Half-life
For a second-order reaction half-life depends on the initial concentration and becomes larger as time goes on.
Again, assuming that [A]t = ½[A]o after one half-life, it can be shown:
o]A[k1
t21
Each succeeding half-life is twice the length of its predecessor.
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343434343434
Graphing Kinetic Data
In addition to the method of initial rates, discussed earlier, rate laws can be deduced by graphical methods.
Note that the zero-order concentration-time equation can be identified as the equation of a straight line.
ot ]A[kt]A[
y = mx + b
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353535353535
Graphing Kinetic Data
In addition to the method of initial rates, discussed earlier, rate laws can be deduced by graphical methods.
Note that the zero-order concentration-time equation can be identified as the equation of a straight line.
This means if you plot [A] vs. time you will get a straight line for a zero-order reaction.
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363636363636
Graphing Kinetic Data
In addition to the method of initial rates, discussed earlier, rate laws can be deduced by graphical methods.
If we rewrite the first-order concentration-time equation in a slightly different form, it can be identified as the equation of a straight line.
kt]A[]A[
lno
t
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373737373737
Graphing Kinetic Data
In addition to the method of initial rates, discussed earlier, rate laws can be deduced by graphical methods.
If we rewrite the first-order concentration-time equation in a slightly different form, it can be identified as the equation of a straight line.
kt]Aln[]Aln[ ot
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383838383838
Graphing Kinetic Data
In addition to the method of initial rates, discussed earlier, rate laws can be deduced by graphical methods.
If we rewrite the first-order concentration-time equation in a slightly different form, it can be identified as the equation of a straight line.
ot ]Aln[kt]Aln[
y = mx + b
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393939393939
Graphing Kinetic Data
In addition to the method of initial rates, discussed earlier, rate laws can be deduced by graphical methods.
If we rewrite the first-order concentration-time equation in a slightly different form, it can be identified as the equation of a straight line.
This means if you plot ln[A] vs. time you will get a straight line for a first-order reaction. (see Figure 13.9)
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Plot of log [N2O5] versus time.
Time (s) [N2O5] log[N2O5]
0 0.0165 1.783
600 0.0124 -1.907
1200 0.0093 -2.032
1800 0.0071 -2.149
2400 0.0053 -2.276
3000 0.0039 -2.409
3600 0.0029 -2.538
)g(O)g(NO4)g(ON2 2252
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Figure 13.9
The figure displayed shows a plot of log [N2O5] at various times during the decomposition reaction. The fact that the points lie on a straight line is confirmation that the rate law is first order.
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424242424242
Graphing Kinetic Data
In addition to the method of initial rates, discussed earlier, rate laws can be deduced by graphical methods.
If we rewrite the second-order concentration-time equation in a slightly different form, it can be identified as the equation of a straight line.
ot ]A[1
kt]A[
1
y = mx + b
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434343434343
Graphing Kinetic Data
In addition to the method of initial rates, discussed earlier, rate laws can be deduced by graphical methods.
If we rewrite the second-order concentration-time equation in a slightly different form, it can be identified as the equation of a straight line.
This means if you plot 1/[A] vs. time you will get a straight line for a second-order reaction.Figure 13.10 illustrates the graphical method of deducing the order of a reaction.
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Time (s) (A) log[NO2] (B) 1/[NO2]
0 -2.000 100
60 -2.166 146
120 -2.286 193
180 -2.379 239
240 -2.456 286
300 -2.521 332
360 -2.578 379
Figure 13.10 Plotting the data for the decomposition of nitrogen dioxide at 330°C.
(g)O + 2NO(g) (g)2NO 22
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Plot of log [NO2] against time. Note that a straight line does not fit the points well.
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Plot of 1/[NO2] against time. Note how closely thepoints follow the straight line, indicating that the
decomposition is second order.
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474747474747
Homework
Chapter 13 Homework: collected at the first exam.
Review Questions: 8.Problems: 51, 53, 57.
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484848484848
Operational Skills
Using the concentration-time equation for first-order reactions
Relating the half-life of a reaction to the rate constant
Time for a few review questions.
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