Consider the following chemical reaction A B+C A plot of In A vs. time (in seconds) is a straight line with a slope of -0.0033 1/s (OF per second). Calculate the time required, in seconds, for the concentration of A to decrease to 1.06 M when the initial concentration of A is 2.06 M
Consider the following chemical reaction A B+C A plot of In A vs. time (in seconds) is a straight line with a slope of -0.0033 1/s (OF per second). Calculate the time required, in seconds, for the concentration of A to decrease to 1.06 M when the initial concentration of A is 2.06 M
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
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![Consider the following chemical reaction
A B+C
A plot of In A vs. time (in seconds) is a straight line with a slope of -0.0033 1/s (OR
per second).
Calculate the time required, in seconds, for the concentration of A to decrease to
1.06 M when the initial concentration of A is 2.06 M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F65e6630c-4421-4972-a63a-fb1641ac4f7a%2F69e40240-329c-4bee-88be-382b8f7693b9%2Fc4bwvsc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Consider the following chemical reaction
A B+C
A plot of In A vs. time (in seconds) is a straight line with a slope of -0.0033 1/s (OR
per second).
Calculate the time required, in seconds, for the concentration of A to decrease to
1.06 M when the initial concentration of A is 2.06 M
Expert Solution
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Step 1
The given graph suggest that reaction is first order.
The rate constant k = - slope
Thus rate constant for given reaction = 0.0033 1/s
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Solved in 2 steps
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