1. The folowing kinetic data were obtained for the reaction between nitric oxide and hydrogen at 7000C Initial conc./mol.dm-3 Initial rate/ mol dm-3 s-1 NO H2 0.01 0.005 0.025 2.4 10-6 0.025 1.2 10^-6 0.0125 0.01 0.6 10^-6 a. The order of the reaction with respect to each reactant; b. The rate constant of the reaction at 7000C (Avery, 24) 2. The recombination of lodine atoms in the gas phase in the presence of Argon was investigated and the order of the reaction was determined by the method of initial rates. The initial rates of reaction of 21(g) + Ar(g) [1]0/ (10-5 mol dm-3) v0/ (mol dm-3 s-1 12(g) + Ar(g) were as follows: 1.0 2.0 4.0 6.0 (a) 8.7 10-4 3.48 10-3 1.39 10-2 3.13 10-2 (b) 4.35 10-3 1.74 10-2 (c) 8.69 10-3 3.47 10-2 The Ar concentrations are (a) 1.0 mmol dm-3, (b) 5.0 mmol dm-3, and (c) 10.0 mmol dm-3. Determine the orders of reaction with respect to the I and Ar atom concentration and the 6.96 10-2 1.57 10-1 3.13 10-1 1.38 10-1 rate constant. (PW. Attkins, 797)
1. The folowing kinetic data were obtained for the reaction between nitric oxide and hydrogen at 7000C Initial conc./mol.dm-3 Initial rate/ mol dm-3 s-1 NO H2 0.01 0.005 0.025 2.4 10-6 0.025 1.2 10^-6 0.0125 0.01 0.6 10^-6 a. The order of the reaction with respect to each reactant; b. The rate constant of the reaction at 7000C (Avery, 24) 2. The recombination of lodine atoms in the gas phase in the presence of Argon was investigated and the order of the reaction was determined by the method of initial rates. The initial rates of reaction of 21(g) + Ar(g) [1]0/ (10-5 mol dm-3) v0/ (mol dm-3 s-1 12(g) + Ar(g) were as follows: 1.0 2.0 4.0 6.0 (a) 8.7 10-4 3.48 10-3 1.39 10-2 3.13 10-2 (b) 4.35 10-3 1.74 10-2 (c) 8.69 10-3 3.47 10-2 The Ar concentrations are (a) 1.0 mmol dm-3, (b) 5.0 mmol dm-3, and (c) 10.0 mmol dm-3. Determine the orders of reaction with respect to the I and Ar atom concentration and the 6.96 10-2 1.57 10-1 3.13 10-1 1.38 10-1 rate constant. (PW. Attkins, 797)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please help me for number 1 and 2
![ll 4G ll 7,1K/s
23:40
TR 02 Kinetika Ki...
TR 02
1. The folowing kinetic data were obtained for the reaction between nitric oxide and hydrogen
at 7000C
Initial conc./mol.dm-3 Initial rate/ mol dm-3 s-1
NO
H2
0.025
0.01
2.4 10^-6
0.025
0.0125
a. The order of the reaction with respect to each reactant;
b. The rate constant of the reaction at 7000C (Avery, 24)
0.005
1.2 10^-6
0.01
0.6 10^-6
The recombination of Iodine atoms in the gas phase in the presence of Argon was
invest
initial rates of reaction of 21(g) + Ar(g)
2.
and the order of the reaction was determined by the method of initial :
The
12(g) + Ar(g) were as follows:
6.0
3.13 10-2
1.0
(1J0/ (10-5 mol dm-3)
v0/ (mol dm-3 s-1
2.0
4.0
1.39 10-2
6.96 10-2
1.38 10-1
(a) 8.7 10-4
3.48 10-3
(b) 4.35 10-3
(c) 8.69 10-3
1.74 10-2
1.57 10-1
3.47 10-2
3.13 10-1
The Ar concentrations are (a) 1.0 mmol dm-3, (b) 5.0 mmol dm-3, and (c) 10.0 mmol dm-3.
Determine the orders of reaction with respect to the I and Ar atom concentration and the
rate constant. (PW. Attkins, 797)
3. For general reaction aA + bB products, the following initial rates are determined
experimentally when reactions are set up with the initial amounts indicated in units of
molarity, M.
[A] (M)
1.44
[B] (M)
Initial rate (M/s)
0.35
3.37 10^-3
1.44
0.70
2.15 10^-2
2.89
0.35
2.69 10^-3
Asumming that the rate law can be written as Rate = k [A]^m. [B]^n
Determine the value of m, n, and k. (Ball, 684)
4. The following results were obtained for the decomposition of glucose in aqueous solution.
54.2
52.5
(G]/ 10^-3 M 56.0
t/ min
55.3
49.0
45
120
240
480
Show that the reaction is first order and calculate the rate constant for the process and the
half-life for glucose uder these conditions. (Avery, 13)
5. The following data were obtained for the hidrolysis of a sugar in aqueous solution at 230C
Time/ min
60
130
180
(S] M
Show that the rection is first order and calculate the rate constant for the hydrolysis.
(Avery, 25)
1.000
0.807
0,630
0.531](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F519feced-309c-4e75-a5b0-166c3bcfbe07%2F650f3215-b1fd-44ee-a20f-3ed9b6e29010%2Fn500v66_processed.jpeg&w=3840&q=75)
Transcribed Image Text:ll 4G ll 7,1K/s
23:40
TR 02 Kinetika Ki...
TR 02
1. The folowing kinetic data were obtained for the reaction between nitric oxide and hydrogen
at 7000C
Initial conc./mol.dm-3 Initial rate/ mol dm-3 s-1
NO
H2
0.025
0.01
2.4 10^-6
0.025
0.0125
a. The order of the reaction with respect to each reactant;
b. The rate constant of the reaction at 7000C (Avery, 24)
0.005
1.2 10^-6
0.01
0.6 10^-6
The recombination of Iodine atoms in the gas phase in the presence of Argon was
invest
initial rates of reaction of 21(g) + Ar(g)
2.
and the order of the reaction was determined by the method of initial :
The
12(g) + Ar(g) were as follows:
6.0
3.13 10-2
1.0
(1J0/ (10-5 mol dm-3)
v0/ (mol dm-3 s-1
2.0
4.0
1.39 10-2
6.96 10-2
1.38 10-1
(a) 8.7 10-4
3.48 10-3
(b) 4.35 10-3
(c) 8.69 10-3
1.74 10-2
1.57 10-1
3.47 10-2
3.13 10-1
The Ar concentrations are (a) 1.0 mmol dm-3, (b) 5.0 mmol dm-3, and (c) 10.0 mmol dm-3.
Determine the orders of reaction with respect to the I and Ar atom concentration and the
rate constant. (PW. Attkins, 797)
3. For general reaction aA + bB products, the following initial rates are determined
experimentally when reactions are set up with the initial amounts indicated in units of
molarity, M.
[A] (M)
1.44
[B] (M)
Initial rate (M/s)
0.35
3.37 10^-3
1.44
0.70
2.15 10^-2
2.89
0.35
2.69 10^-3
Asumming that the rate law can be written as Rate = k [A]^m. [B]^n
Determine the value of m, n, and k. (Ball, 684)
4. The following results were obtained for the decomposition of glucose in aqueous solution.
54.2
52.5
(G]/ 10^-3 M 56.0
t/ min
55.3
49.0
45
120
240
480
Show that the reaction is first order and calculate the rate constant for the process and the
half-life for glucose uder these conditions. (Avery, 13)
5. The following data were obtained for the hidrolysis of a sugar in aqueous solution at 230C
Time/ min
60
130
180
(S] M
Show that the rection is first order and calculate the rate constant for the hydrolysis.
(Avery, 25)
1.000
0.807
0,630
0.531
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