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George Mason University Crystal Violet Dye Reaction Order Lab Report

George Mason University Crystal Violet Dye Reaction Order Lab Report

Question Description

I’m studying for my Chemistry class and don’t understand how to answer this. Can you help me study?

Make the three graphs below on excel, Include a picture of the excel graphs on a word doc as well because my excel is old.

After consulting the table of reaction orders and their attributes, the order of the crystalviolet dye should make itself apparent if, after collecting the absorbance and time data, threegraphical plots are prepared for each trial:

• One graph of absorbance vs. time

• One graph of ln(absorbance) vs. time

• One graph of 1/absorbance vs. time

Only one type of these plots should be a straight line. This is therefore a direct, graphicaldetermination of the order of reaction with respect to crystal violet dye.

Discussion:

1. What is the order of the reactant crystal violet?

2. Compare the values for slope from the linear graphs you obtained. Does there appear to be any trendyou can spot when comparing these two slopes and the change in concentration of hydroxide ion?Rates of reaction should be proportional to observed values for k.

3. In general, which of the two concentrations reached the 90% mark more quickly? State any trend thatstands out.

4. The starting concentration (time zero) of crystal violet is 1 x 10-4 M. Using the proper integratedrate law and the calculated value for k, calculate the concentration of crystal violet after 240 seconds.

5. Use the y-intercept from your straight line to obtain a value for e0, the extinction coefficient, forcrystal violet at time zero. Use the Beer-Lambert Law to do this.

Data Table: Chemical kinetics: Crystal Violet Dye

Concentration of NaOH solution

0.0251 NaOH

Concentration of Crystal Violet Dye Solution

0.001M

Room Temperature (assumed to be reaction temperature)

Trial #1

Trial #2

Time (sec)

%T

Time (min)

%T

30

0.970

30

1.019

60

0.861

2

0.913

90

0.767

90

0.809

120

0.676

120

0.716

150

0.590

150

0.624

180

0.516

180

0.540

210

0.444

210

0.467

240

0.383

240

0.402

270

0.327

270

0.344

300

0.280

300

0.297

330

0.239

330

0.255

360

0.206

360

0.219

390

0.173

390

0.189

420

0.150

420

0.165

450

0.131

450

0.146

Data Table continued

Concentration of NaOH solution

0.05051

Concentration of Crystal Violet Dye Solution

0.001M

Room Temperature (assumed to be reaction temperature)

Trial #1

Trial #2

Time (sec)

%T

Time (min)

%T

30

1.025

30

0.471

60

1.020

60

0.372

90

1.021

90

0.294

120

1.018

120

0.232

150

1.016

150

0.182

180

1.014

180

0.140

210

1.012

210

0.109

240

1.008

240

0.085

270

1.006

270

0.067

300

1.001

300

0.052

330

0.998

330

0.042

360

0.993

360

0.031

390

0.991

390

0.025

420

0.989

420

0.020

450

0.986

450

0.016

Also Include 1-5 sentences that briefly summarize the procedureand what information was obtained

■ Example:– ____ g (or mL) of Reagent A were reacted with _____ g (or mL) ofReagent B until a precipitate formed/gas evolved/color changeoccurred. Observations were made and data were collected. Table 1represents _____. Table 2 represents _____. Figure 1 represents_____. Figure 2 represents ____.

and include a conclusion:

Restate the purpose of the experiment

■ How did you attempt to meet the purpose?

■ Was the purpose met?

■ Restate the anticipated outcome. Was the actual outcome close tothe anticipated outcome?

■ Why or why not? What errors did you specifically experience inthis experiment?– Distance-learning format of the class is not an error

■ What are some future improvements to this experiment?– “Updating the lab manual”, “clear/better instructions onhow to perform calculations”, “instructor not explaining thelab procedure”, “do not make the class a distance-learningcourse”, etc. are NOT future improvements

Let me know if you have any questions!

lab report below pages 186-194


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