RD Lab - Exp-05 - G-A1.pdf
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The document describes a laboratory experiment to determine the reaction order and rate constant of the reaction between sodium hydroxide (NaOH) and ethyl acetate (CH3COOC2H5). The group prepared 0.1 M solutions of each reactant and mixed them in a batch reactor at room temperature while measuring conductivity over time. Calculations using the conductivity readings showed the reaction was second order. The rate constant was determined to be 1.291651 × 10-3 at 21°C based on the nonlinear ln(CA/CAo) vs time graph.
![7
1. Draw: Ln (CA/CAo) vs time
The curve is nonlinear so assume that is second order reaction.
So, k calculated by:
ln
CA
CAo
= −Kt
At t = 60s → ln
0.046271394
0.05
= −K × 60 → K = 1.291651 × 10-3 at 21 oC
Then, we can find out Rate of reaction (r) from reaction rate law equation:
−ra = K × [CA]α
r = 1.291651 × 10-3 × [0.046271394]2
r = 2.7654 × 10-6
M/sec
-0.12
-0.1
-0.08
-0.06
-0.04
-0.02
0
0 10 20 30 40 50 60 70 80 90 100 110 120 130
Axis
Title
Axis Title
Ln(CA/CAo) vs t](https://image.slidesharecdn.com/rdlab-exp-05-g-a1-220618165814-1639eff5/85/RD-Lab-Exp-05-G-A1-pdf-9-320.jpg)
![8
2. 1/CA vs time
This is the first order because is linear (but we have some error in the recording
data) and k can calculate by slope or below eq.:
1
CA
−
1
CAo
= Kt
At t = 60s
1
0.046271394
−
1
0.05
= K × 60
K = 0.02686
−ra = K × [CA]α
ra = 0.02686 × [0.046271394]1
ra = 1.2428 * 10-3
18.5
19
19.5
20
20.5
21
21.5
22
22.5
0 10 20 30 40 50 60 70 80 90 100 110 120 130
1/CA
Time (s)
1/CA vs Time](https://image.slidesharecdn.com/rdlab-exp-05-g-a1-220618165814-1639eff5/85/RD-Lab-Exp-05-G-A1-pdf-10-320.jpg)
RD Lab - Exp-05 - G-A1.pdf
- 1. Koya University Faculty of Engineering Chemical Engineering Department 3rd Stage (2021-2022) Reactor Laboratory Lab Report Number of Experiment: 5 Experiment Name: Rate Law of Reaction Experiment Date: 10/11/2021 Submitted on: 17/11/2021 Instructor: Mr. Ahmed Abdulkareem Ahmed Group: A1 Prepared by: Safeen Yaseen Jafar Rivan Dler Ali Ramazan Shkur Kakl Rokan Mohammad Omer Ibrahim Ali Ahmed Mamand Aziz
- 2. Table of Content Aim of Experiment......................................................................................................................................1 Procedure.....................................................................................................................................................2 Tools and Apparatus...................................................................................................................................3 Table of Reading .........................................................................................................................................5 Calculation and Results..............................................................................................................................6 Discussion ..................................................................................................................................................10
- 3. 1 1. Aim of Experiment ➢ To determine the reaction order. ➢ To find out the reaction constant (K).
- 4. 2 2. Procedure 1. Prepare 1 L and 0.1 M of NaOH liquid (solution). after it, we need to prepare second reactant for reaction occur prepare 1 L and 0.1 M of CH3COOC2H5 solution . 2. First of all, in the service units close all valve if open. After that put the bottles in specific places in service unit. And be careful to that the pipes and valves are connected as well. 3. Turn on the switch control box (power supply). 4. This experiment operates in the room temperature (at 21 oC in this experiment). 5. Set the limited flow rate of the reagents before run the steps. 6. Switch on the valves and pumps of reactants 7. Take the reactants from their containers (bottles to the first). 8. We fill the reactor by both reactant liquids and the flow rate would be limited at both flow meters in the control box. 9. Switch on the stirrer from the main control box. 10. Turn on the conductivity meter (which connected initially to the reactor). 11. Feeds continuously enter the reactor and out the reactor. 12. The conductivity measurements (Conductivity sensor) must be noted while change of the conductivity reach the constant value. The readings should be taken at every 10 second. 13.At the end of the experiment, turn off the pumps, stirrer. 14. Turn off the power of control interface box. 15. Reactants should be removed from both (1 and 2) reactant bottle container. Then, the liquids must be kept for following test.
- 5. 3 3. Tools and Apparatus Figure 2: Service Unit - Back Part Figure 1: Service Unit - Front Part 1 2 4 3 5 6 7 Figure 3: Control Unit 8 10 11 12 Figure 4: Batch Reactor
- 6. 4 Service Unit, control unit and its parts: 1. Water Bath: is the tank which contain water it used for control temperature of reactants. 2. Water Bath temperature switch button and controllers. 3. Reactant Container 1: For storage reactant 1. 4. Reactant Container 2: For storage reactant 2. 5. Water Pump AB-1: it used for pumping water. 6. Pump AB-2: It used for pump the reactor 1. 7. Pump AB-3: It used for pump the reactor 2. 8. Pump AB-1 on/off button: It used for switch on or switch of pump AB-1. 9. Power Button: Used to turn on control unit. 10. Temperature Display: For displaying the temperatures 11. Speed Controller: For control the velocity of reactant. 12. Sensor Selector: it used for select the temperature sensor that you want. Batch reactor parts: 1. Coil: for control the temperature of the reaction. 2. Conductivity Sensor: for record the conductivity. 3. Temperature Sensor: for record temperature. 4. Stirrer: for mix the reactants and make a collision for reactants.
- 7. 5 4. Table of Reading Time (s) Conductivity or 𝛌 (mS) 𝛌𝐨 𝛌∞ 0 11.46 11.46 3.28 10 10.68 11.46 3.28 20 10.84 11.46 3.28 30 10.85 11.46 3.28 40 10.84 11.46 3.28 50 10.87 11.46 3.28 60 10.85 11.46 3.28 70 10.85 11.46 3.28 80 10.85 11.46 3.28 90 10.85 11.46 3.28 100 10.84 11.46 3.28 110 10.84 11.46 3.28 120 10.82 11.46 3.28 130 10.84 11.46 3.28 140 3.28 11.46 3.28 *T = 21 oC
- 8. 6 5. Calculation and Results Concentration for each 10 sec. can calculated by this equation: CA CAo = λo− λ λo− λ∞ Conversion calculated by this equation: X = CAo−CA CAo We can find out the order of the reaction and constant (K) of the reaction by know linear or non-linear below equations: ln CA CAo = −Kt 1 CA − 1 CAo = Kt Time (sec) Conductivity (mS) Concentration Ln(CA/CAo) 1/CA 0 11.46 0.05 0 20 10 10.68 0.045232274 -0.10021215 22.10811 20 10.84 0.046210269 -0.07882096 21.64021 30 10.85 0.046271394 -0.077499083 21.61162 40 10.84 0.046210269 -0.07882096 21.64021 50 10.87 0.046393643 -0.074860559 21.55468 60 10.85 0.046271394 -0.077499083 21.61162 70 10.85 0.046271394 -0.077499083 21.61162 80 10.85 0.046271394 -0.077499083 21.61162 90 10.85 0.046271394 -0.077499083 21.61162 100 10.84 0.046210269 -0.07882096 21.64021 110 10.84 0.046210269 -0.07882096 21.64021 120 10.82 0.04608802 -0.081469969 21.69761 130 10.84 0.046210269 -0.07882096 21.64021 140 3.28 0 #NUM! #DIV/0!
- 9. 7 1. Draw: Ln (CA/CAo) vs time The curve is nonlinear so assume that is second order reaction. So, k calculated by: ln CA CAo = −Kt At t = 60s → ln 0.046271394 0.05 = −K × 60 → K = 1.291651 × 10-3 at 21 oC Then, we can find out Rate of reaction (r) from reaction rate law equation: −ra = K × [CA]α r = 1.291651 × 10-3 × [0.046271394]2 r = 2.7654 × 10-6 M/sec -0.12 -0.1 -0.08 -0.06 -0.04 -0.02 0 0 10 20 30 40 50 60 70 80 90 100 110 120 130 Axis Title Axis Title Ln(CA/CAo) vs t
- 10. 8 2. 1/CA vs time This is the first order because is linear (but we have some error in the recording data) and k can calculate by slope or below eq.: 1 CA − 1 CAo = Kt At t = 60s 1 0.046271394 − 1 0.05 = K × 60 K = 0.02686 −ra = K × [CA]α ra = 0.02686 × [0.046271394]1 ra = 1.2428 * 10-3 18.5 19 19.5 20 20.5 21 21.5 22 22.5 0 10 20 30 40 50 60 70 80 90 100 110 120 130 1/CA Time (s) 1/CA vs Time
- 11. 9
- 12. 10 6. Discussion Discussion – Safeen Yaseen Ja’far In this experiment as in experiment of the batch reactor (conversion test) we calculate the conductivity and concentration by time (10 to 10 sec.) until we reach a constant value of the conductivity. Then, by the equation and graphs determine/find out the value of 𝛂 by know the linearity of the graphs then by given equation or graphs slope we found out K value also by reaction rate law found rate of the reaction. But because of the error in this exp. Because of conductivity sensor doesn’t work properly it cause to wrong value or mistake in recording data of conductivity. Then the equations that use to find k maybe give us the wrong value.
- 13. 11 Discussion – Rivan Dler Ali Prepare the solution NaOH and CH3COOC2H5 and put into the batch reactor. And start the reaction by turn on the stirrer. But we use different conductivity meter because level of the solution is low and batch reactor conductivity meter didn’t reach to the conductivity sensor. After that we start record of the conductivity with time and convert it to ln(Ca/Ca0) and 1/Ca. from the table we can understand that conductivity and concentration decrease when time passes but the ln(Ca/Ca0) and 1/Ca is proportional with time. in the ln(Ca/Ca0) with time graph shows that the ln(Ca/Ca0) at first 10 seconds ln(Ca/Ca0) decrease when time passes, but between 10-20 seconds ln(Ca/Ca0) increases after that become stable. at second graph which shows the relationship between 1/Ca and time. we can understand from the graph the first 10 seconds the 1/Ca increase and between 10- 20 decrease and after that point the 1/Ca become stable with time.
- 14. 12 Discussion – Ibrahim Ali In this experiment we prepare the of solution of sodium hydroxide and ethyl acetate it consists of water and inter the batch reactor to mixing the solution and then the aim of this experiment is to determine the reaction (K) and reaction order. When the process is start, we reading the conductivity of solution and we notice when the conductivity with time is indirectly change and concentration with time is indirectly change In this experiment in the first step we didn’t have the liner line so we can find the rate of reaction by the equation
- 15. 13 Discussion – Ahmed Mamand Aziz In this experiment we must be known that we have a room temperature condition. Our data (on the reaction of 0.1M NaOH and O.1M CH3COOHC2H5). And we recorded some value of conductivity according to time. By using the little low that written of our report we could found the Conversion. If we see the table, we will know the relationship between (conductivity-conversion} both with time, and in the graphs we know that the relation between (cond. and time) is opposite, meaning that conductivity will decrease according to time. And we know that the relationship between (CA/Cao and time) is opposite, meaning that CA/CAo will decrease when the time will pass. and the relationship between (1/CA and time) is also proportional, meaning the 1/CA will increase when the time pass.
- 16. 14 Discussion – Rokan Mohammad At the first Prepare 1 L and 0.1 M of NaOH liquid (solution). after it, we need to prepare second reactant for reaction occur prepare 1 L and 0.1 M of CH3COOC2H5 solution . and put In the Bach reactor and turn on stirer this experiment we must be known that we have a room temperature condition. And we recorded some value of conductivity according to time. By using the little low that written of our report we could found the Conversion. If we see the table and graph, we will know the relationship between (conductivity-conversion} both with time, and in the graphs we know that the relation between (cond. and time) is opposite, meaning that conductivity will decrease according to time. And we know that the relationship between (CA/Cao and time) is opposite, meaning that CA/CAo will decrease when the time will pass. and the relationship between (1/CA and time) is also proportional, meaning the 1/CA will increase when the time pass. And in this experiment, we should use different conductivity meter. Beacouse the level of solution is low doesn’t reach the conductivity meter.
- 17. 15 Discussion – Ramazan Shkur Kakl Prepare the NaOH and CH3COOC2H5 solution and place it in the batch reactor. Turn on the stirrer to start the reaction. However, because the solution level is low and the batch reactor conductivity meter did not reach the conductivity sensor, we used a different conductivity meter. Following that, we begin recording conductivity with time and converting it to ln(Ca/Ca0) and 1/Ca. As seen in the table, conductivity and concentration drop as time passes, while ln(Ca/Ca0) and 1/Ca remain proportionate to time. The ln(Ca/Ca0) with time graph indicates that the ln(Ca/Ca0) decreases for the first 10 seconds as time passes, but then climbs over the next 10-20 seconds before being steady. The connection between 1/Ca and time is seen in the second graph. The graph shows that the 1/Ca increases for the first 10 seconds, then decreases for the next 10-20 seconds, before stabilizing with time.