ergy. When the reactant Are pre. Cooled it slows the reaction so you Are Able to do experiments 4. The data show an initial change in crystal violet concentration (A[CV+]/At) with time after mixing crystal violet and OH. From the equation for the trendline, calculate the rate of the reaction, including units. The reaction is CV+ + OH → CVOH. [CV]= =X [CV*] (M) y=-1.832E-8x + 1.013E-5 R²= 0.987 time (s) 5. For the figure in 4., draw a line to show the predicted results if the experiment is repeated at a higher temperature with the same initial concentration of CV+.
ergy. When the reactant Are pre. Cooled it slows the reaction so you Are Able to do experiments 4. The data show an initial change in crystal violet concentration (A[CV+]/At) with time after mixing crystal violet and OH. From the equation for the trendline, calculate the rate of the reaction, including units. The reaction is CV+ + OH → CVOH. [CV]= =X [CV*] (M) y=-1.832E-8x + 1.013E-5 R²= 0.987 time (s) 5. For the figure in 4., draw a line to show the predicted results if the experiment is repeated at a higher temperature with the same initial concentration of CV+.
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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![In Kinetic energy
When the reactant Are pre. Cooled it slows the reaction so you
Are Able to do experiments
4. The data show an initial change in crystal violet concentration (A[CV+]/At) with time after mixing
crystal violet and OH. From the equation for the trendline, calculate the rate of the reaction, including
units. The reaction is CV+ + OH → CVOH.
[CV]-x
=X
[CV] (M)
y=-1.832E-8x + 1.013E-5
R²= 0.987
time (s)
5. For the figure in 4., draw a line to show the predicted results if the experiment is repeated at a higher
temperature with the same initial concentration of CV*.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F51a557d3-dfa2-4172-8fc3-d4922b05ac41%2Fedf2cd02-5c67-49e5-b763-a0fb68c2ae00%2Fa92tfeg_processed.jpeg&w=3840&q=75)
Transcribed Image Text:In Kinetic energy
When the reactant Are pre. Cooled it slows the reaction so you
Are Able to do experiments
4. The data show an initial change in crystal violet concentration (A[CV+]/At) with time after mixing
crystal violet and OH. From the equation for the trendline, calculate the rate of the reaction, including
units. The reaction is CV+ + OH → CVOH.
[CV]-x
=X
[CV] (M)
y=-1.832E-8x + 1.013E-5
R²= 0.987
time (s)
5. For the figure in 4., draw a line to show the predicted results if the experiment is repeated at a higher
temperature with the same initial concentration of CV*.
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