Given the data given from the first page, how would I plot a Beer's Law Plot on the second page with the grid
![Beer's Law Plot
Absorbance
M
[Cu*2] unknown: Method a =
Method b =](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0ea55b65-6a30-46ce-96b8-2b732a599bb3%2Fe13be72b-1f38-45f0-af49-4d7acde12660%2Fgdydccr_processed.jpeg&w=3840&q=75)
![Beer's Law
Beer's Law Plot
1.40
1.20
1.00
0.80
0.60
0.40
0.20
0.00
.02
.04
.06
.08
.1
Concentration (M)
Experimental Data:
[Cu*2]
.100 M
Absorbance
1.20
.080 M
0.97
.060 M
0.70
.040 M
0.50
.020 M
0.25
.000 M
0.00
Absorbance](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0ea55b65-6a30-46ce-96b8-2b732a599bb3%2Fe13be72b-1f38-45f0-af49-4d7acde12660%2Fakrhtm_processed.jpeg&w=3840&q=75)
Lambert-Beer’s law is one of the most important rules in the chapter of photochemistry. The mathematical form of the law is given as follows:
Here, ‘A’ is the absorbance, ‘c’ is the concentration of the sample solution, and is a constant known as molar absorptivity coefficient, and ‘l’ is the path length.
From, this relation it is clear that the absorbance is directly proportional to the concentration of the sample solution.
That means if the concentration increases, the absorbance will increase and vice-versa.
Thus, if we plot absorbance (along y axis) vs. concentration (along x axis), we are expected to get a straight line passing through the origin.
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