The reaction described by the equation O₂(g) + NO(g) → O₂(g) + NO₂(g) has, at 310 K, the rate law rate of reaction = = K[03][NO] k= 3.0 x 106 M-¹.s-¹ Given that [0₂] = 3.0 x 10-4 M and [NO] = 5.0 x 10-5 M at t = 0, calculate the rate of the reaction at t = 0. rate: 0.072 Incorrect M/S
The reaction described by the equation O₂(g) + NO(g) → O₂(g) + NO₂(g) has, at 310 K, the rate law rate of reaction = = K[03][NO] k= 3.0 x 106 M-¹.s-¹ Given that [0₂] = 3.0 x 10-4 M and [NO] = 5.0 x 10-5 M at t = 0, calculate the rate of the reaction at t = 0. rate: 0.072 Incorrect M/S
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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![The reaction described by the equation
O₂(g) + NO(g) - O₂(g) + NO₂(g)
has, at 310 K, the rate law
rate of reaction = k[03][NO] k = 3.0 x 106 M-¹.S-¹
Given that [03] = 3.0 × 10 M and [NO] = 5.0 × 10-5 M at t = 0, calculate the rate of the reaction at t = 0.
rate:
0.072
Incorrect
What is the overall order of this reaction?
1
2
0
M/s](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9437567b-8da5-455d-a4fe-2bd0f454b63f%2F79a18bc6-d3ef-4129-95ec-f436a41a535f%2F1ktoy3u_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The reaction described by the equation
O₂(g) + NO(g) - O₂(g) + NO₂(g)
has, at 310 K, the rate law
rate of reaction = k[03][NO] k = 3.0 x 106 M-¹.S-¹
Given that [03] = 3.0 × 10 M and [NO] = 5.0 × 10-5 M at t = 0, calculate the rate of the reaction at t = 0.
rate:
0.072
Incorrect
What is the overall order of this reaction?
1
2
0
M/s
Transcribed Image Text:Ⓒ Macmillan Learning
The rate constant for this zero-order reaction is 0.0230 M-s¹ at 300 °C.
A →→ products
How long (in seconds) would it take for the concentration of A to decrease from 0.800 M to 0.320 M?
x10
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