The reaction 2A + 2B → M + N has the rate law: Rate = k[A]2. At 25°C, k = 0.0110 L mol-1 s-1. If the initial concentrations of A and B are 0.363 M and 0.509 M, respectively What is the half-life of the reaction? What will be the concentrations of A and B after 30.0 minutes?
The reaction 2A + 2B → M + N has the rate law: Rate = k[A]2. At 25°C, k = 0.0110 L mol-1 s-1. If the initial concentrations of A and B are 0.363 M and 0.509 M, respectively What is the half-life of the reaction? What will be the concentrations of A and B after 30.0 minutes?
Chemistry
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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
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The reaction 2A + 2B → M + N has the rate law: Rate = k[A]2. At 25°C, k = 0.0110 L mol-1 s-1. If the initial concentrations of A and B are 0.363 M and 0.509 M, respectively
What is the half-life of the reaction?
What will be the concentrations of A and B after 30.0 minutes?
![The reaction 2A + 2B → M+ N has the rate law: Rate = k[A]?. At 25°C, k = 0.0110 L mol 1s1. If the initial concentrations of A and
0.363 M and 0.509 M, respectively
Bare
X Your answer is incorrect.
(a)
What is the half-life of the reaction?
seconds
Hint
Assistance Used
Use the integrated form of the second-order rate law. The final concentration will be one-half of the initial concentration.
X Your answer is incorrect.
(b)
What will be the concentrations of A and B after 30.0 minutes?
[A] = i
M
[B] = i
M
Hint
Assistance Used
Use the integrated rate law for a 2nd order reaction to find the amount of A that reacts. Then use stoichiometry to convert
from the amount of A that reacts to the amount of B that reacts.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8ad36720-6101-4e4b-abcd-9f36fc84b0e9%2F615bf2ef-330c-4c04-96ac-e62e6cc632a1%2F695szq_processed.png&w=3840&q=75)
Transcribed Image Text:The reaction 2A + 2B → M+ N has the rate law: Rate = k[A]?. At 25°C, k = 0.0110 L mol 1s1. If the initial concentrations of A and
0.363 M and 0.509 M, respectively
Bare
X Your answer is incorrect.
(a)
What is the half-life of the reaction?
seconds
Hint
Assistance Used
Use the integrated form of the second-order rate law. The final concentration will be one-half of the initial concentration.
X Your answer is incorrect.
(b)
What will be the concentrations of A and B after 30.0 minutes?
[A] = i
M
[B] = i
M
Hint
Assistance Used
Use the integrated rate law for a 2nd order reaction to find the amount of A that reacts. Then use stoichiometry to convert
from the amount of A that reacts to the amount of B that reacts.
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