1. Using the following chemical equation and data: 3A+B+2CD +2E Experiment Initial [A] Initial [B] Initial [C] Initial Rate 1 1.0 x 10² 4.0 x 10 2.0 x 10² 5 mM/s 2 1.0 x 102 8.0 x 10-³ 2.0 x 10-2 10 mm/s 3 2.0 x 10-² 8.0 x 10-³ 2.0 x 10-² 40 mm/s 4 2.0 x 10² 8.0 x 10-³ 1.0 x 10² 40 mm/s a. Determine the rate equation. b. Calculate the specific rate constant (k). c. Determine the initial rate of reaction if the initial concentrations of A, B, C are 3 x 10-² M, 5 x 10-³ M, 5 x 10-5 M, respectively, for the reaction.
1. Using the following chemical equation and data: 3A+B+2CD +2E Experiment Initial [A] Initial [B] Initial [C] Initial Rate 1 1.0 x 10² 4.0 x 10 2.0 x 10² 5 mM/s 2 1.0 x 102 8.0 x 10-³ 2.0 x 10-2 10 mm/s 3 2.0 x 10-² 8.0 x 10-³ 2.0 x 10-² 40 mm/s 4 2.0 x 10² 8.0 x 10-³ 1.0 x 10² 40 mm/s a. Determine the rate equation. b. Calculate the specific rate constant (k). c. Determine the initial rate of reaction if the initial concentrations of A, B, C are 3 x 10-² M, 5 x 10-³ M, 5 x 10-5 M, respectively, for the reaction.
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![Kinetics Problems Laboratory
1. Using the following chemical equation and data:
3A + B + 2CD +2E
Experiment
Initial [A]
Initial [B]
Initial [C]
Initial Rate
1
1.0 x 10²
4.0 x 10-³
2.0 x 10²
5 mM/s
2
1.0 x 10-²
8.0 x 10-³
2.0 x 10-²
10 mm/s
3
2.0 x 10-²
8.0 x 10-³
2.0 x 10-²
40 mm/s
4
2.0 x 10-²
8.0 x 10-³
1.0 x 10-²
40 mM/s
a. Determine the rate equation.
b. Calculate the specific rate constant (k).
c. Determine the initial rate of reaction if the initial concentrations of A, B, C are
3 x 10-2 M, 5 x 10-³ M, 5 x 10-5 M, respectively, for the reaction.
2. The reaction between bromate ions and bromide ions in acidic aqueous solution is given
by the following equation:
BrO³- (aq) + 5Br (aq) + 6H* (aq) → 3Br2 (1) + 3H₂O (1)
The experimental results are given below. Using these data, determine the orders for
all reactants, the overall reaction order, and the value of the rate constant.
Experiment
Initial
Initial
Initial
Initial Rate
[BrO³-]
[Br]
[H+]
(Ms¹)
1
0.10
0.10
0.10
8.0 x 104
2
0.20
0.10
0.10
1.6 x 10-³
3
0.20
0.20
0.10
3.2 x 10-³
4
0.10
0.10
0.20
3.2 x 10-³](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F06775211-663a-4915-8f33-409e31fb1882%2F6640b388-6b1d-4f07-970a-38fec9fcc3b5%2Fom2cw5q_processed.png&w=3840&q=75)
Transcribed Image Text:Kinetics Problems Laboratory
1. Using the following chemical equation and data:
3A + B + 2CD +2E
Experiment
Initial [A]
Initial [B]
Initial [C]
Initial Rate
1
1.0 x 10²
4.0 x 10-³
2.0 x 10²
5 mM/s
2
1.0 x 10-²
8.0 x 10-³
2.0 x 10-²
10 mm/s
3
2.0 x 10-²
8.0 x 10-³
2.0 x 10-²
40 mm/s
4
2.0 x 10-²
8.0 x 10-³
1.0 x 10-²
40 mM/s
a. Determine the rate equation.
b. Calculate the specific rate constant (k).
c. Determine the initial rate of reaction if the initial concentrations of A, B, C are
3 x 10-2 M, 5 x 10-³ M, 5 x 10-5 M, respectively, for the reaction.
2. The reaction between bromate ions and bromide ions in acidic aqueous solution is given
by the following equation:
BrO³- (aq) + 5Br (aq) + 6H* (aq) → 3Br2 (1) + 3H₂O (1)
The experimental results are given below. Using these data, determine the orders for
all reactants, the overall reaction order, and the value of the rate constant.
Experiment
Initial
Initial
Initial
Initial Rate
[BrO³-]
[Br]
[H+]
(Ms¹)
1
0.10
0.10
0.10
8.0 x 104
2
0.20
0.10
0.10
1.6 x 10-³
3
0.20
0.20
0.10
3.2 x 10-³
4
0.10
0.10
0.20
3.2 x 10-³
![3. The decomposition of N₂O5 in the gas phase was studied at constant temperature,
2N₂O5 (g) → 4NO2 (g) + O2(g)
The following results were collected:
[N₂Os]
Ln[N₂Os]
Time (s)
0.1000
0
0.0707
50
0.0500
100
0.0250
200
300
0.0125
0.00625
400
a. Complete the table. Using the data and graph paper, plot the [N₂O3] versus time and
Ln[N₂O5] versus time. Determine the value of k. Which graph did you use?
b. On your graph of [N₂Os] versus time, highlight the times it takes for each halving of
the reactant concentration. What is the half-life? Using this half-life calculate k.
4. Using the Arrhenius equation, one can design experiments to find the activation energy,
Ea.
k = Ae-Ea/RT
or by setting up this equation to find Ea:
k₁
Ea
In
=
-K (21/12 - 1)
k₂
R\T₂
Using the following data for the N₂O5 decomposition, calculate the average E₁ using at least 3
values of Ea to find the average and standard deviation.
T (°C)
k(s¹)
2.0 x 10-$5
T(K)
20
7.3 x 10-5
30
2.7 x 10-4
40
9.1 x 10-4
50
2.9 x 10-³
60
Note the value of R is 8.3144 J/K mol.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F06775211-663a-4915-8f33-409e31fb1882%2F6640b388-6b1d-4f07-970a-38fec9fcc3b5%2Fnvc3009_processed.png&w=3840&q=75)
Transcribed Image Text:3. The decomposition of N₂O5 in the gas phase was studied at constant temperature,
2N₂O5 (g) → 4NO2 (g) + O2(g)
The following results were collected:
[N₂Os]
Ln[N₂Os]
Time (s)
0.1000
0
0.0707
50
0.0500
100
0.0250
200
300
0.0125
0.00625
400
a. Complete the table. Using the data and graph paper, plot the [N₂O3] versus time and
Ln[N₂O5] versus time. Determine the value of k. Which graph did you use?
b. On your graph of [N₂Os] versus time, highlight the times it takes for each halving of
the reactant concentration. What is the half-life? Using this half-life calculate k.
4. Using the Arrhenius equation, one can design experiments to find the activation energy,
Ea.
k = Ae-Ea/RT
or by setting up this equation to find Ea:
k₁
Ea
In
=
-K (21/12 - 1)
k₂
R\T₂
Using the following data for the N₂O5 decomposition, calculate the average E₁ using at least 3
values of Ea to find the average and standard deviation.
T (°C)
k(s¹)
2.0 x 10-$5
T(K)
20
7.3 x 10-5
30
2.7 x 10-4
40
9.1 x 10-4
50
2.9 x 10-³
60
Note the value of R is 8.3144 J/K mol.
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