CHEM 112A Midterm: chem112A-fa2011-mt2-Francis-soln

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turquoisegnu128

8 Jan 2019

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Please provide all answers in the spaces provided. You are not allowed to use a calculator for this exam, but you may use molecular model kits. Including the title page, there should be 11 total questions spread over 6 pages. There is also a seventh page that should be blank. You can use this last page for scratch paper if you need it, but please remem- ber to copy your answers into the blanks that are provided for each question. 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Related Questions

PROCEDURES :

Rinse and flush a burette with the solution of NaOH provided and set it up. Fill the burette with the solution of NaOH solution.

Using a 15-mL volumetric pipette, collect an accurate volume of the 0.1 M HC1 solution and add it to a 250-mL beaker that contains about 50-mL of deionized water and a magnetic stir bar. Place the beaker on a stir plate and begin stirring.

Turn on the Vernier LabQuest by pressing the silver power button in the upper left corner. Connect a pH probe into the slot marked CH 1, this slot is located on the top edge of the LabQuest. The LabQuest will automatically recognize the type of probe and begin to display the pH data.

Using the stylus provided tap the tabs displayed at the top of the screen to toggle between the Meter screen, Graph screen and Data Table screen.

Conduct the titration by adding the basic solution from the burette to the acid solution. You should take the pH reading after every addition of I.00 mL of the base solution. Continue the titration process until you have added 30.00 mL of the base solution.

Rinse the probe several times with tap water followed with deionized water.

Insert the clean probe you just rinsed in the acid solution labelled X and determine its pH.

Insert the clean probe you just rinsed in the base solution labelled Y and determine its pH.

Dispose the waste according in the labeled waste disposal container.

graph of pH vs. volume of NaOH solution added that will be graded according to the graph guidelines provided below;

GRAPH GUIDELINES

Submit a FULL PAGE OF titration curve by stapling it to this report sheet. Your graph will be graded based on the âChemistry Graph Checklistâ posted on Blackboard, which includes overall appearance. You may seek out help from peers while learning to use Excel, but your graph must be your own.

1. Appropriate tittle (5 points)

2. Correct labelling of both axes (10 points)

3. Correct units on both axes (10 points)

4. Graph occupying at least Â¾ of the page used (5 points)

5. Correct scales for both axes (10 points)

6. General shape of the graph (10 points)

Please someone helps me I did it but i dont know what im missing

can someone complate what I miss

Can someone please paraphrase this to me in short sentences...

1. Obtain a benzoic acid pellet, determine the mass of the pellet on the analytical balance and record the mass in your hard covered note book. The error for the analytical balance is ï± 0.0005 g. Attach approximately 10.0 cm of fuse wire as shown by your Instructor (use the length of the card that holds the fuse wire, the card is already calibrated in heat units, cal or 4.18 J units) and adjust it to give firm contact with the benzoic acid pellet. Avoid kinks in the fuse wire.

2. Carefully assemble the bomb, keeping surfaces of closure scrupulously clean. Dismantled parts should be placed on a clean, dry paper towel. Place the bomb on the bench next to the O2 cylinder. Tighten cover by hand. The Instructor must assist you in connecting the bomb to the O2 cylinder, and slowly admit oxygen to a final pressure of 20 atm (280 psi.) Close valves on cylinder. Relieve pressure in line by means of the black knob on the regulator. Remove the gas coupling and check the circuit again.

3. Place the bomb in the calorimeter and make sure the ignition wires are connected properly. Carefully fill the inner reservoir in the calorimeter with 2000 mL distilled water, using the volumetric flask provided. The water should completely cover the bomb; no oxygen bubbles should escape from the bomb if the seal is good. If there is a substantial leak, the bomb should be dried and refilled with oxygen. Small leaks are insignificant.

4. Connect the motor and pulley experiment with the o-ring provided and starts the stirrer. Connect the leads on the outside of the bomb jacket to the 10 cm fuse in the igniter

. 5. Turn on the stirrer. For this, data points should be collected every ten seconds up to a total of 150 data points.

6. After at least 12 data points have been collected, and the temperature is reasonably constant or shows only a small up- or downward trend, press and hold the ignition button on the ignitor for approximately 1second. You will see the red light on the ignition box flash on and off again, showing that the fuse wire has burned. You should NOT be standing over the bomb while igniting the bomb!! Stand back from the bomb for at least 15 seconds. If combustion has occurred, the temperature will start to rise within the next two or three data points.

7. Keep recording data until the 150 points finishes.

8. Remove the bomb from the calorimeter and relieve the pressure by opening the valve. BE SURE to open the release valve before trying to unscrew the top of the bomb! 9. Measure the remaining length of unoxidized fuse wire. (This information is needed to correct for its heat of combustion). Carefully clean and dry the calorimeter and sample pan.

10. Repeat this procedure with the second benzoic acid pellet.

11. Once you have good data for benzoic acid, allowing you to calculate the calorimeter constant C, repeat the full procedure for each of the two sucrose samples.

Experiment 1: Calculating Rate of Reaction

In this experiment you will calculate the rate of reaction of potassium iodide and hydrogen peroxide. The order of the reaction will also be determined.

Materials:

20 mL 3% Hydrogen peroxide, H₂O₂
15 mL Iodine-Potassium Iodide Solution, IKI (1% Iodine, 2% Potassium Iodide)
100 mL Beaker
10 mL Graduated cylinder
100 mL Graduated cylinder
250 mL Beaker
(2) 250 mL Erlenmeyer flasks
1-Hole Rubber stopper
2-Hole Rubber stopper
(2) 3 in. Rigid tubing pieces
(1) 6 in. Rigid tubing
6 Pipettes

Stopwatch
Permanent marker
Waste beaker (any volume)
*Access to graphing software
*Access to a computer
*24 in. Flexible tubing
*Water
*10 mL Distilled water

* You must provide

*You must cut this piece of tubing into two, 12 inch pieces. (if you have not already done so).

Procedure

Preparation of Apparatus

Set up apparatus as shown in Figure 2. To do this, begin by labeling the Erlenmeyer Flasks as 1 and 2. The reaction will take place in Flask 1.

Fill Flask 2 approximately three quarters of the way full with water.

Press the 2-hole rubber stopper into the top of Flask 2. Place one three in. piece and one six in. piece of rigid tubing into each hole of the rubber stopper. This should create an airtight system.

Place the one-hole stopper on Flask 1, and fit the remaining 3 in. piece of rigid tubing in the stopper hole.

Connect Flask 1 and Flask 2 with the two, 12 in flexible tubing pieces. One piece should connect Flask 1 to Flask 2, and the second piece should connect Flask 2 to the graduated cylinder. The tubing which connects Flask 2 to the graduated cylinder should be positioned low enough to be immersed in the water in Flask 2.

Figure 2: Apparatus set-up. Note this is a sample set-up and is not drawn to scale. Your specific equipment may vary slightly.

Part A: Preparation of Reactants

Pour five mL of the IKI solution into a 10 mL graduated cylinder.

Add five mL of distilled water to the graduated cylinder to bring the total volume to 10 mL. This is the 0.5% - 1.0% (diluted) IKI solution.

Pour 15 mL of 3% H₂O₂ solution into a 100 mL beaker.

Add five mL of distilled water to this beaker and mix with a stir rod. This is the 2.25% (diluted) H₂O₂ solution.

Part B: Performing the Reaction

Remove the stopper from Flask 1 and place five mL of the 3% (undiluted) H2O2 solution and 10 mL of the undiluted IKI solution provided into the flask. Immediately replace the stopper on the flask.
Note: At this point, you should select an extra beaker (any volume) from your lab kit to use as an supplemental collection container beaker for Step 6. You do not need to use the beaker yet, but keep it in close proximity.

Swirl Flask 1 until you observe a steady dripping of water going into the 10 mL graduated cylinder. This could take 3 - 5 minutes. Check for leaks in the tubing or system if water does not start rising up the plastic tubing coming from Flask 2 and traveling towards the graduated cylinder within one minute.

Stop swirling Flask 1 when you notice the steady flow of water droplets. When you stop, the water drop -rate will significantly decrease (to around one drop every 5 - 20 seconds) and could take a few minutes to stabilize. If a steady flow of drops of water does not occur within a few minutes, swirl Flask 1 for 1 more minute and check again. Repeat this process until there is a steady flow of drops of water after you have stopped swirling Flask 1.

Quickly empty liquid that has collected in the 10 mL graduated cylinder and replace the empty cylinder back under the flexible tubing.

Allow the flow of drops to become steady again. This could take 1 - 3 mL of water.

Start timing once the drop rate is steady and the volume of water collected is at a whole number (such as three mL). Record the time in Table 1 each time 2 mL of is water displaced. Continue taking data until you have at least 10 data points (20 mL displaced).
Note: Use the extra beaker (located in Part B: Step 1) to collect additional fluid when the volume of displaced water exceeds 10 mL.

Return the collected water from your 10 mL graduated cylinder to Flask 2. Ensure the seal is air tight.

Empty, clean and dry Flask 1 and the graduated cylinder.

Repeat Steps 1 - 8 for the following trial conditions: 5 mL 3% (undiluted) H₂O₂ mixed with 10 mL of 0.5%-1.0% IKI solution (placed in Flask 1); and, 5 mL of 2.25% H₂O₂ mixed with 10 mL of 1.0%-2.0% IKI solution (placed in Flask 1). Record the data in Table 2 and Table 3, respectively.
Note: Clean the graduated cylinder and extra collection beaker before it is used to measure any additional reagents for Trial 2 or Trial 3; and, before it is used for collecting the water from the reaction in the apparatus.

Use a graphing software program to make a graph of each trial. The graph should demonstrate the relationship formed between time vs. mL of water displaced.

Find and record the slope and the inverse slope for each trial.

Table 1: 10 mL Undiluted (1.0 -2.0%) IKI and 5 mL 3% H₂O₂
mL water displaced	Time (seconds)
2
4
6
6
8
10
12
14
16
18
20
22
Slope:
Inverse Slope:

Table 2: 10 mL Diluted (0.5-1.0% IKI) and 5 mL 3% H₂O₂
mL water displaced	Time (seconds)
2
4
6
6
8
10
12
14
16
18
20
22
Slope:
Inverse Slope:

Table 3: 10 mL Undiluted (1.0 -2.0%) IKI and 5 mL 2.25% H₂O₂
mL water displaced	Time (seconds)
2
4
6
6
8
10
12
14
16
18
20
22
Slope:
Inverse Slope:

Calculations

Post-Lab Questions

1. Determine the order of the KI in this reaction.

2. Determine the order of the H2O2 in this reaction.

3. Calculate the rate law constant.

4. What is the overall rate law?

5. When finding the order of H2O2, why was Trial 1 and Trial 3 used?

6. When finding the order of KI, why was Trial 1 and Trial 2 used?

7. Research and identify some alternative catalysts that could be used to accelerate the decomposition of hydrogen peroxide. Evaluate these catalysts and determine which option is

CHEM 112A Midterm: chem112A-fa2011-mt2-Francis-soln

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