4.2b: Differential Rate Law Snow Day

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Ancillary Documents

UALR Students Use Documents in Google Classroom The following links allow anyone to make their own copy of the assignment, which they can modify and reuse, but students must use the copies provided in Google Classroom for grading.

Copy of Worksheet I: Kinetics (Group Activity)
Lab Report Page: Includes procedures, class data sheet, and Lab Report Template

Learning Objectives

Students will be able to:
Content

Design a series experiments to calculate the constants involved in function, the rate law, where the value of the dependent variable (Rate Law) depends on three independent variables (concentration of two reactions and temperature).
Apply this to the reaction of the reduction of Ferric Iron by Iodide at various temperatures.
Understand how the initial rate of a chemical reaction producing iodine can be measured in an iodine clock reaction.
Work up the data and calculate the rate constant at room temperature, the order of reaction with respect to Ferric and Iodide ions and the Arrhenius constant from rate law data.
Understand the mathematics of all the calculations

Process

Run experiments to measure the initial rate of reaction by varying three independant variables, [Fe⁺²], [I^-] and T.
Use a spreadsheet to calculate the order of reaction from log log plots of Rate and concentration data.
Use a spreadsheet to calculate the Arrhenius constant from temperature and ln rate constant data.
Report results

Prior Knowledge

Redox Reactions (LibreText Section 3.6)
Use of Logarithms (LibreText Section 14.0.2)
Use of spreadsheets on log and natural log plots (Graphing Lab)
Use of spreadsheet functions (Graphing Lab)

Recommended Prior Reading

Worksheet II: The Experiment

The second part of the lab will go over running the experiment and working up the data. Do to winter weather you will not be able to mix actual reagents but we will go over the procedures and you are responsible for understanding basic laboratory techniques like reading a burette, along with safe operating procedures like wearing safety glasses. In the real lab students would work in groups of two, mix the solutions and record the time it takes for the solution to turn blue. There is an element of error intrinsic error in the data of this lab, as for example, we are basing the reaction time on a subjective observation, when a solution turns blue. That is, two students who are looking at the exact same reaction might record different times because they interpret different shades of blue to indicate the reaction is over. Likewise, inconsistent mixing could induce error both within experiments of a group, and across groups. If these errors are random in contrast to systematic (see section 1B.2), the effects can be minimized by running lots of experiments, and so the class would all share their data. So we will watch three videos, one of each experiment and record the time to turn blue, and then add that data to a data set created by a previous class, and then like the previous class, work up the entire data set (including the values we contributed with our observations of the videos).

There are two approaches to working up large sets of data, convert the measured values to average values and plot that, or use spreadsheets to calculate the multiple values and then plot all of the data. In lab 2 we were introduced to the use of equations on Google Sheets, and in this lab we will build a Workbook in Google Sheets where we not only work up all the data, but create a dashboard on the front page of the workbook and then create a separate sheet within the workbook for each of the three experiments we ran, showing all calculations involved in each graph. Therefore, in addition to Worksheet II students will need to develop and submit a workbook in Google Sheets and unlike the first worksheet, this is an individual assignment where each student submits an individual worksheet and workbook, although students are encouraged to work these up as teams, but each student needs to submit their own workbook and worksheet for grading.

Part V: Obtaining the Data

In part IV you designed the three experiments needed to run to obtain the constants (m, n and E_A). The following table shows 5 experimental conditions where 50 mL of the two reagents were mixed and the time was recorded until the solution turned blue. Students work in groups and share their data. Each experiment is identified by an experiment number (1-5) and table \(\PageIndex{1}\) shows the concentrations and volumes of reagents mixed. Students will work this data up with three graphs.

Graph 1: Experiments 1-3: Order of rxn with respect to [Fe⁺³ ] at T3 = room, [I^-]= constant.
Graph 2: Experiments 3-5: Order of rxn with respect to [I^-] at T3 = room, [Fe⁺³] = constant
Graph 3: Experiment 3: Arrhenius constant, at different T3 , with [Fe⁺³] and [I^-] held constant

	Reagent 1 250 mL Erlenmeyer Flask				Reagent 2 100 mL Beaker				After Mixing
Exp. #	0.04M Fe⁺³ (mL)	0.15M HNO₃ (mL)	H2O (mL)	Exp. #	0.04M I^- (mL)	0.004M S₂O₃^-2 (mL)	Starch, (mL)	H2O, (mL)	Temp (^oC)
1	20.00	20.00	10.00	1	10.00	10.00	5.00	25.00	room
2	15.00	20.00	15.00	2	10.00	10.00	5.00	25.00	room
3	10.00	20.00	20.00	3	10.00	10.00	5.00	20.00	room or variable
4	10.00	20.00	15.00	4	15.00	10.00	5.00	15.00	room
5	10.00	20.00	10.00	5	20.00	10.00	5.00	15.00	room

Table 1: volumes and concentrations of solutions mixed in the different experimental runs

You goal is to calculate the Rate at t=0 (moment of mixing) as the reaction starts the moment the two solutions are mixed. If both of the above flasks have 50 mL the total of the combined solution will be 100 mL. To calculate the concentration of any reagent at the moment of mixing you use the dilution equation, please review section 4.4.3

\[M_iV_i=M_fV_f\]

Where M_i is the initial Molarity (added to either reagent flask), V_i is the initial volume (added to either reagent flask), M_f is the final molarity (in the reaction flask) and V_f is the final volume of the mixture (100 ml). So

\[M_f=M_i \frac{V_i}{V_f}\]

note, the term \(\frac{V_i}{V_f}\) is often called the dilution factor, and is dimensionless if both volumes have the same units.

These concentrations need to be calculated for both reactants ([Fe+3] and [I-]) in each experiment along with the thiosulfate concentration ([S₂O₃^-2]) that is used to calculate the initial rate. Figure 2 shows the table of the Google Doc where you post the ferric iron and iodide concentrations.

Before proceeding complete activities 1 and 2 of the Google Doc associated with this activity if assigned

Part VI: The Data

The following table provides a experimental data that was pooled by a class. The trial number represents the number of times the students repeated an experiment and the experiment number is aligned with the concentrations used in table 2 of figure 2 (above). You should plot all the data in your google sheets workbook (not use average values) and experiment 3 room temperature data should be used in all three graphs.

Trial #	Exp. #	Time (s)	Temp (^oC)	Group #	Exp. #	Time (s)	Temp (^oC)
1	1	29.45	22.90	2	4	75.03	22.90
2	1	32.36	22.90	3	4	77.78	22.90
3	1	29.88	22.90	4	4	67.82	22.90
4	1	29.32	22.90	5	4	79.97	22.90
Video	1		22.90	6	4	67.56	22.90
1	2	52.03	22.90	Video	4		22.90
2	2	54.69	22.90	1	5	52.90	22.90
3	2	52.60	22.90	2	5	55.10	22.90
4	2	55.29	22.90	3	5	66.44	22.90
5	2	56.50	22.90	4	5	65.90	22.90
6	2	50.00	22.90	5	5	57.10	22.90
7	2	52.60	22.90	6	5	53.29	22.90
Video	2		22.90	Video	5		22.90
1	3	120.01	22.90	1	3, T_Cold	254.85	16.30
2	3	121.12	22.90	2	3, T_Cold	265.52	19.90
3	3	126.33	22.90	3	3, T_Cold	242.79	17.30
4	3	129.56	22.90	4	3, T_Cold	438.20	14.20
5	3	118.14	22.90	Video	3, T_Cold		21.40
6	3	125.69	22.90	1	3, THot	13.55	35.30
7	3	128.55	22.90	2	3, THot	20.97	35.80
Video	3		22.90	3	3, THot	20.32	34.90
1	4	72.59	22.90	Video	3, THot		25.01
				Video	3, THot		30.67

The following videos were taken of various solutions and you need to watch them and insert into the spreadsheet the missing data

Video \(\PageIndex{5}\): Iodine Clock Experiment 1 (V.S. Belford) https://youtu.be/jJUeYYhNdvA	[Fe⁺³] = 0.008M	Video \(\PageIndex{4}\): Iodine Clock Experiment 2 (V.S. Belford) https://youtu.be/OCzPDUk6Tks	[Fe⁺³] = 0.006M
	[ I^-] = 0.004M		[ I^-] = 0.004M
	[S₂O₃^-2] = 0.0004M		[S₂O₃^-2] = 0.0004M
	T = 22.90 ℃		T = 22.90 ℃

Video \(\PageIndex{3}\): Iodine Clock Experiment 3 (V.S. Belford) https://youtu.be/ec4fKe38Agg	[Fe⁺³] = 0.004M	Video \(\PageIndex{2}\): Iodine Clock Experiment 4 (V.S. Belford) https://youtu.be/ZaudifbeKwg	[Fe⁺³] = 0.004M
	[ I^-] = 0.004M		[ I^-] = 0.006M
	[S₂O₃^-2] = 0.0004M		[S₂O₃^-2] = 0.0004M
	T = 22.90 ℃		T = 22.90 ℃

Video \(\PageIndex{1}\): Iodine Clock Experiment 5 (V.S. Belford) https://youtu.be/M1JpDpBuTUM	[Fe⁺³] = 0.004M	Video \(\PageIndex{6}\): Iodine Clock Experiment 3 at T=21.40 ℃ (V.S. Belford) https://youtu.be/OCzPDUk6Tks	[Fe⁺³] = 0.004M
	[ I^-] = 0.008M		[ I^-] = 0.004M
	[S₂O₃^-2] = 0.0004M		[S₂O₃^-2] = 0.0004M
	T = 22.90 ℃		T = 21.40 ℃

Video \(\PageIndex{1}\): Iodine Clock Experiment at T=25.01 ℃ (V.S. Belford) https://youtu.be/6jHEFzBGL8o	[Fe⁺³] = 0.004M	Video \(\PageIndex{2}\): Iodine Clock Experiment at T=30.67 (V.S. Belford) https://youtu.be/OCzPDUk6Tks	[Fe⁺³] = 0.004M
	[ I^-] = 0.004M		[ I^-] = 0.004M
	[S₂O₃^-2] = 0.0004M		[S₂O₃^-2] = 0.0004M
	T = 25.01℃		T = 30.67 ℃

The Failed Experiment

In this video a student forgot a reagent, can you figure out which one?

Answer: Thiosulfate, the reaction instantly turns blue as there is no thiosulfate to stop iodine from accumulating.

Part VII: Working up the Data and Google Sheets Workbooks

There are three graphs we need to plot, the first two deal with the power function relationships of the constant temperature rate law (eq. 4.2) and the third deals with the temperature dependence of the rate constant (eq. 4.3)

Figure \(\PageIndex{3}\): Basic plots we will use in this lab. (Belford, cc.0)

Use the regular Lab Page