Initial Rates Question: Note dm³ = L Nitrogen(II)oxide reacts with hydrogen as shown by the following equation. 2NO(g) + 2H₂(g) → N₂(g) + 2H₂O(g) The table below shows how the rate of reaction varies as the reactant concentrations vary. Experiment 1 2 3 4 Initial [NO] / Initial [H₂]/ moldm mol dm 0.100 0.100 0.100 0,200 0.200 0.100 0.300 0.100 Initial rate/ mol N₂ dms 2.53x10 5.05x10 10.10x10 22.80x10* a) Determine the order with respect to NO and to H2 and write the rate law b) Explain how you determined the order for NO c) What is the value of k (include units)
Initial Rates Question: Note dm³ = L Nitrogen(II)oxide reacts with hydrogen as shown by the following equation. 2NO(g) + 2H₂(g) → N₂(g) + 2H₂O(g) The table below shows how the rate of reaction varies as the reactant concentrations vary. Experiment 1 2 3 4 Initial [NO] / Initial [H₂]/ moldm mol dm 0.100 0.100 0.100 0,200 0.200 0.100 0.300 0.100 Initial rate/ mol N₂ dms 2.53x10 5.05x10 10.10x10 22.80x10* a) Determine the order with respect to NO and to H2 and write the rate law b) Explain how you determined the order for NO c) What is the value of k (include units)
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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![Initial Rates Question: Note dm³ = L
Nitrogen(II)oxide reacts with hydrogen as shown by the following equation.
2NO(g) + 2H₂(g) → N₂(g) + 2H₂O(g)
The table below shows how the rate of reaction varies as the reactant concentrations vary.
Experiment
1
2
3
4
Initial [NO] / Initial [H₂] /
mol dm
mol dm³
0.100
0.100
0.200
0.300
0.100
0.200
0.100
0.100
A suggested mechanism for this reaction is as follows.
Initial rate/
mol N₂ dms
H₂+NOX fast step
X+NO→Y+H₂O slow step
Y+H₂ → N₂ + H₂O fast step
2.53x106
5.05x10*
a) Determine the order with respect to NO and to H2 and write the rate law
b) Explain how you determined the order for NO
c) What is the value of k (include units)
10.10x10
22.80x10**
d) State and explain if this mechanism agrees with your experimental rate law](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F21ed1cfb-364f-46d5-bbe5-45039b5aabf3%2F54afe2c2-4cb1-4f8d-ade9-7f1916cea20c%2Fjcln9s_processed.png&w=3840&q=75)
Transcribed Image Text:Initial Rates Question: Note dm³ = L
Nitrogen(II)oxide reacts with hydrogen as shown by the following equation.
2NO(g) + 2H₂(g) → N₂(g) + 2H₂O(g)
The table below shows how the rate of reaction varies as the reactant concentrations vary.
Experiment
1
2
3
4
Initial [NO] / Initial [H₂] /
mol dm
mol dm³
0.100
0.100
0.200
0.300
0.100
0.200
0.100
0.100
A suggested mechanism for this reaction is as follows.
Initial rate/
mol N₂ dms
H₂+NOX fast step
X+NO→Y+H₂O slow step
Y+H₂ → N₂ + H₂O fast step
2.53x106
5.05x10*
a) Determine the order with respect to NO and to H2 and write the rate law
b) Explain how you determined the order for NO
c) What is the value of k (include units)
10.10x10
22.80x10**
d) State and explain if this mechanism agrees with your experimental rate law
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