CHEM 102 University Of California Chemical Kinetics Lab Report One file is for Lab Report Guidleines and one is an example lab report. These are the lab i

CHEM 102 University Of California Chemical Kinetics Lab Report One file is for Lab Report Guidleines and one is an example lab report.

These are the lab instructions:

In this experiment, the source of SO32– will come from sodium sulfite, Na2SO3, in the starch solution. When the sulfite ion (SO32–) reacts with the iodate ion (IO31–), it will produce iodine (I2). The iodine (I2) will then form a complex with starch, and produce a dark-blue color. This dark-blue complex can be used as an indicator to indicate the completion of the reaction.

The reaction order with respect to one of the reactants in the rate law can be determined by keeping the concentrations of all of the other reactants in the rate law, constant. In this experiment, there will be a total of four runs, each with a different initial concentration of iodate ion (IO31–). The concentration of iodate (IO31–) will be varied, while the concentration of the only other reactant, the sulfite ion (SO32–), in the rate law will be kept constant.

Watch the experiment demonstration, and write a lab report using the data plot the time and concentration for both the 1st Order and 2nd Order plots, as described in Chapter 13, section 13.4 “Graphing Kinetic Date”. Choose the best-fit line to determine the Reaction Order. Then using the slope of the plot chosen, determine the value of the Rate Constant.

Youtube video for data and demonstration:

https://www.youtube.com/watch?v=dkzWCNupemU&feature=emb_title Jane Smith
Lab Partner: John Doe
Lab Performed: 7/17 & 7/19
Introduction
Chemistry 102
LATTC
Summer 2020
Lab 1: Simple Distillation and Fractional Distillation
Distillation is a technique that allows for the separation and purification of a mixture of liquids
that have different boiling points. This process involves heating the mixture to different boiling
points. Liquids must be distilled from the lowest boiling point to the highest boiling point.
Heating the liquid to its boiling point causes the liquid to transform into the vapor phase where it
can then be recondensed into its liquid form. The sequence can then be continued to distill
liquids at higher boiling points.
There are four different types of distillation: simple, fractional, steam, and vacuum. This
experiment details both simple and fractional distillation. In a simple distillation, vapors pass
immediately into the condenser, where they cool, condense and are passed into the receiving
flask. Depending on the composition of the vapors at a given temperature and pressure, distilling
via simple distillation might not be pure. For this reason, simple distillation is typically used to
separate liquids with significantly different boiling points.
Fractional distillation is used when the boiling points of two liquids is very close. This technique
separates the components with repeated vaporization-condensation cycles within the
fractionating column.
Methods and Materials
The following materials were used to complete the simple distillation:
? Heating apparatus
? Round bottom flask
? Thermometer
? Cold water condenser
? Rubber tubes
? Graduated cylinder or collection flask
? Clamps
? Stand
? Joint grease
To complete the fractional distillation the above listed materials were used in addition to a
fractionating column.
1
Procedure:
The following procedure was used to complete the experiment:
Simple Distillation:
1. Assemble apparatus for simple distillation:
a. Connect the condenser, to the chamber with the thermometer. Be sure to grease
all joints. Connect the rubber tubes to the condenser and establish a water flow,
ensuring there are no air bubbles present. Set up graduated cylinder or receiving
flask at the base of the condenser.
2. Combine 10 mL of rubbing alcohol in a 25 mL round bottom flask. Add a boiling stone.
Fit this boiling stone into the apparatus and fit snugly into the heating element.
3. Turn on the heating element and slowly raise the temperature until the vapors are visible
in the still. Aim for a rate of distillation 1mL per 4 minutes.
4. Record the temperature and time at which the first drop of distillate is produced. Record
the temperature and volume of distillate every 4 minutes.
5. When there is no more distillate produced, turn off the heating element. Raise the
apparatus away from the heating element and allow it to cool to room temperature.
6. Graph the collected data.
Fractional Distillation:
1. Set up the apparatus as instructed above, adding the fractionating column.
2. Repeat the distillation process as described above (recording the volume of the distillate
and temperature every 4 minutes).
3. Plot the results on the same graph as the data from the simple distillation.
Raw Data
Time (Minutes)
Temperature (°C)
Volume Distillate Produced
(mL)
0:00
55
1 drop
1:30
65
0.5 mL
4:30
65
1mL
8:00
74
2 mL
11:21
75
3 mL
2
14:26
76
4 mL
19:28
79
5 mL
23:45
79
5.2 mL
27:25
77
5.25 mL
30:00
80
5.3 mL
Table 1: Recorded volume (mL) and temperature (°C) during simple distillation
Time (Minutes)
Temperature (°C)
Volume Distillate Produced
(mL)
0:00
53
1 drop
2:14
60
1 mL
4:04
63
1.75 mL
5:01
63
2 mL
6:00
63
2.75 mL
7:02
65
3 mL
8:05
65
3.5 mL
9:45
65
4 mL
10:30
65
4.25 mL
11:59
64
5 mL
16:44
59
6 mL
20:37
55
6.2 mL
24:00
55
6.4 mL
26:00
50
6.6 mL
28:00
50
6.6 mL
30
50
6.6 mL
Table 2: Recorded volume (mL) and temperature (°C) during fractional distillation
Results
3
Based on the above data, the following graph was created.
Discussion
The graph and data above indicate that the fractional distillation method was able to distill a
larger amount of the rubbing alcohol. Based on this data, it can be determined that the original
mixture of the solution being distilled wasn’t a full 70% rubbing alcohol. Since only 6.6 mL were
collected out of 10 mL, it is better estimated that the original solution was approximately 66%
rubbing alcohol.
Both the simple distillation and fractional distillation occurred at relatively stable temperatures.
The simple distillation occurred between 55 °C and 80 °C. The fractional distillation occurred
between 53 °C and 64 °C. The difference in distillation temperatures could be attributed to the
technique. For the fractional distillation, the liquid vaporizes and then passes through a tall
fractionated column where it then condenses and evaporates until the rubbing alcohol is
completely separated from the water in the mixture.
When it comes to simple distillation, there is a much smaller distance for the vapors to travel and
therefore may result in a less pure substance. In this regard, the simple distillation should have
theoretically produced more distillate than the fractional distillation, since the fractional
distillation should have resulted in a more pure substance.
4
There are a number of reasons that could contribute to this inaccuracy, which all generally come
back to human error. Firstly, the initial measurement in the simple distillation could have been
inaccurate. Instead of starting with a full 10 mL it is possible that a lesser amount was measured
and used to begin the distillation.
Secondly, in order to complete a successful distillation that results in a pure substance,
maintaining a consistent temperature is very important. In the case of the simple distillation there
was a much greater range of temperature than when the fractional distillation was completed.
This could be due to the fact that the simple distillation is a smaller column so it is more subject
to changes in heat. Alternatively, the apparatus could have been transferring an inconsistent
amount of heat. Another possibility is that the temperature was increased too quickly due to
impatience.
Conclusion
Based on the data collected it can be determined that the percentage composition of the original
solution was approximately 66% rubbing alcohol as compared to the labeled 70% rubbing
alcohol.
5
Lab Guideline for Chem 102 (Los Angeles Trade Tech College)
Title: Title of lab experiment and experiment number
Name: Your name
Lab partner: __________
Introduction: Provide background and clearly state the goal of the experiment (1 or 2 paragraphs)
Methods and Materials: List critical materials, chemicals, glassware, equipment, and techniques needed
to perform the experiment.
Procedure: Include relevant information needed to perform experiment. Outline or flow chart format.
Raw Data (This is collected During the Lab Experiment).
Record data (with units) and observations in the lab notebook. This data will be used to write and
complete the Lab Report.
1. Use black or blue ball point pen only.
2. Record data/observations directly into the lab notebook.
Examples:
Empty flask = 23.5 g
(using Mettler Toledo AL104 balance)
Flask + distilled water = 50.3 g
After adding 0.1 g of sodium metal (solid) to water 10.4 mL): reaction occurred
giving off heat, fire, noise, etc.
3. Must be clear and readable.
4. Students may perform experiments in a group (2 per group), but each student must enter data into
his/her notebook. At the end of lab each student must hand in a duplicate notebook sheet containing
the recorded data (doesn’t have to be neat, but must be readable).
Results: This is the manipulated data; the calculated results. The result you got from the individual data.
Includes raw data/observations collected during the experiment and calculations.
Data: Organize the data collected during the experiment (list, table, or graph format). Use
relevant significant figures and include units (cm, mL, g).
Example:
Table 1. Assay Results.
Reagent
GRX
BRX
Activity
77 %
45%
Purity
82%
50%
X
Figure 1. Plot
Discussion: Were the goals of the experiment achieved? If not – what might have happened that caused
the unexpected outcome (error, technique, laziness, etc.). What could have been done to improve the
experiment? What did you learn? (Discussion should consist of a minimum of 2 paragraphs)
Conclusion: Summarize the outcome of the experiment in 2-5 sentences.

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