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Kinetics Theory Lab
Olivia Downs
3/21/11
CHM 1046L/85606
The purpose of this experiment was to determine rates of iodide ions with peroxodisulfate
ions to calculate orders to find the rate constant “k”. Also, we found the activation energy,
frequency factor, and measured the effect of a catalyst on the rate of reaction.
Data of the effect of a catalyst (Cu(NO3)2) on the reaction
Trial
Temp ˚C
Time(sec)
Avg. Time(sec)
13
25˚C
21.2, 24.1, 24.3
23.2
14
25˚C
47.3, 40.6, 44.6
44.2
15
23˚C
63.0, 58.9, 56.9
59.6
16
23˚C
127.0, 114.0, 112.0
117.7
Data of Part III
Trial
KI
(NH4)2S2O8
Rate avg
Rate constant
(k)
Ratio of k
values
13
.084
.042
2.72E5
7.710E3
k13/k1=0.49
14
.042
.042
1.43E5
8.102E3
k14/k2=1.41
15
.042
.042
1.06E5
1.202E2
k15/k3=2.90
16
.042
.042
5.37E6
1.162E2
k16/k4=3.47
Calculating concentrations of [I], [S2O8^2], [S2O3^2]
M1V1=M2V2 Dilution formula
(.008L)× (.2M) ÷ (.019L) = .084210526
= .084 I^
(.004L)× (.2M) ÷ (.019L) = .042105263
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View Full Document = .042 S2O8^2
= .084 S2O3^2
Calculating the rate with respect to
[S2O3^2]
½ × .084 ÷ 93
=5.54E5 s^1
Calculating the order with respect to [I]
=
2.455530683
=2.4514
Calculating the order with respect to
[S2O8^2]
=
1.148863386
=1.1473
Calculating the rate constant for Trial 1
Rate constant= k ÷ [.084]^1.721[.042]^1.250
(5.54e5) ÷ [.084]^1.721[.042]^1.250
K= 1.571e2 s^1
Complete rate law
Rate law= 5.953e3[I^]^1.721[S2O8]^1.250
Calculating Activation energy
Slope= E(a)/R
Slope × R= Ea
(8.314)(3060.1)= 25442
E(a)= 25442 kJ/mol
Calculating Frequency factor
A= k/e^E(a)/RT
(5.54e5) ÷ e^(25442 ÷ (8.314)(23))
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This note was uploaded on 11/03/2011 for the course CHM 1046L taught by Professor Simmons during the Spring '11 term at Tallahassee Community College.
 Spring '11
 Simmons
 Kinetics

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