Rate Law Expressions For the general reaction, aA (g) + bB (g) ? products, the rate law takes the form: Rate = K[A]m[B]n Where: K = rate constant m and n = order of reaction (if m or n = 0, zero-order reaction takes place; if m or n = 1, first-order reaction if present. Use the data to determine the rate law for the reaction and the rate constant (K): ------( see attached image)-------- Using the given rate law expression: ------( see attached image)-------- 1. Use the data from experiments 1 & 2. 2. As you increase the concentration of CH3I (by the factor of 2) from 0.20 to 0.40, what happens to the initial rate? What is the relationship? 3. Calculate the kinetic order of CH3I using the data on experiments 1 & 2. 1. Use the data from experiments 2 and 3. 2. As you increase (by the factor of 2) the concentration of NaOCH2H5, what happens to the initial rate? What is the relationship? 3. Calculate the kinetic order of NaOCH2H5 using the data on experiments 2 and 3. 4. Calculate the rate constant K, using the results from experiment #1.
Rate Law Expressions
For the general reaction, aA (g) + bB (g) ? products, the rate law takes the form:
Rate = K[A]m[B]n
Where:
K = rate constant
m and n = order of reaction
(if m or n = 0, zero-order reaction takes place; if m or n = 1, first-order reaction if present.
- Use the data to determine the rate law for the reaction and the rate constant (K):
------( see attached image)--------
Using the given rate law expression:
------( see attached image)--------
1. Use the data from experiments 1 & 2.
2. As you increase the concentration of CH3I (by the factor of 2) from 0.20 to 0.40, what happens to the initial rate? What is the relationship?
3. Calculate the kinetic order of CH3I using the data on experiments 1 & 2.
1. Use the data from experiments 2 and 3.
2. As you increase (by the factor of 2) the concentration of NaOCH2H5, what happens to the initial rate? What is the relationship?
3. Calculate the kinetic order of NaOCH2H5 using the data on experiments 2 and 3.
4. Calculate the rate constant K, using the results from experiment #1.
![Rate = k[CH3I]™[NaOC2H5]"
%3D](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F14dc0def-aa4d-479b-8181-01c026b1c8e4%2F0a9b2628-7e99-4ef6-815b-e3393b6f67df%2Frnh9at2_processed.png&w=3840&q=75)
![Initial concentrations
(CH3I]
(M)
(NAOC2H5]
(M)
Expt.
Initial rate
(M Is)
1
0.20
0.10
2.0 x 10-5
2
0.40
0.10
4.0 x 10-5
3
0.40
0.20
8.0 x 10-5
4
0.10
0.20
2.0 x 10-5](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F14dc0def-aa4d-479b-8181-01c026b1c8e4%2F0a9b2628-7e99-4ef6-815b-e3393b6f67df%2Fv4ybopg_processed.png&w=3840&q=75)
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