| 3304ENG/7517ENG – Control SystemsSemester 1, 2012 | | System Response in Time Domain | Name | Student No | Time Slot | Signature | 1 Johan Jarvi | | Monday | | Tuesday | | Wednesday | | Thursday | 13:00 | Friday | | | | 2 Lachlan Hutch | | | | | | | | We, by signing this page, declare that the work presented in this report is all work done by us, unless appropriate reference has been made to the work of others. We acknowledge that should this not be the case the report will receive zero marks and due action may be taken. | | Lab Number: 1 | | | Demonstrator | | Submitted on | | Mark Received | |
1.1. Requirements of Experiment 1 …show more content…
The values of Kp are 0.2576, 0.7727 and 10.3 for T1(s), T2(s) and T3(s) respectively.
1.3. Solution Description
In order to complete the experiment the values for Kp were needed as shown at the end of the previous section. The method of simplify the block diagram in section 1.2 to the final transfer function equation is shown below:
Then by substituting in values for Km, Kθ and τ, gives:
Ts= 155.3Kps2+10s+155.3Kp eq. 1.3.1.
That then is the final version of the simplified equation to get the values for Kp needed in the ESVL section of the experiment.
In order to calculate the response characteristics the equations listed in the introductions were utilized and programmed into the MATLAB program in order to speed up the calculation progress for each of the experiments.
The MATLAB code generated was quite basic, the program aimed to easily calculate the required variables through firstly finding the pole locations using the MATLAB built in abs
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In the experiment we used Turnip, Hydrogen Peroxide, Distilled Water, and Guaiacol as my substances. On the first activity, Effect of Enzyme concentration of Reaction Rate for low enzyme concentration, we tested three concentrations of the turnip extract, and hydrogen peroxide. For the Turnip Extract I used 0.5 ml, 1.0 ml, and 2.0 ml. For hydrogen peroxide we used 0.1 ml, 0.2 ml, and 0.4 ml. We used a control to see the standard, and used a control for each enzyme concentration used. The control contains turnip extract and the color reagent, Guaiacol. We prepared my substrate tubes separately from the enzyme tubes. My substrate tube
My signature indicates that this document represents my own work. Outside of shared data, the information, thoughts and ideas are my own except as indicated in the references. In addition I have not given aid to another student on this assignment.
This is then done for all trials. Then, once all five values of k are found, the average is taken by adding all five values of k and dividing by 5. The experimental k average is 0.105894M/s.
pH was recorded every time 1.00 mL of NaOH was added to beaker. When the amount of NaOH added to the beaker was about 5.00 mL away from the expected end point, NaOH was added very slowly. Approximately 0.20 mL of NaOH was added until the pH made a jump. The pH was recorded until it reached ~12. This was repeated two more times. The pKa of each trial are determined using the graphs made on excel.
To begin, three sets ofabout 0.3000g of KHP are weighed out on an analytical balance. Put the three sets of KHP into three separate, labeled flasks. All three sets of the KHP is then dissolved with approximately 50mL of deionized water. Next, a buret is used to start the actual titration. Buret is initially filled to 0.00mL mark with the NaOH solution, this is recorded as initial volume. Next, add 2-3 drops of phenolphthalein indicator into each of the three flasks containing KHP. A magnetic stir bar is then added to the first flask, and placed above a stir plate. Everything is positioned under the buret. Stirrer is put on medium speed and the titration can start. Slowly release the NaOH into the KHP flask. As the end point is reached, a pink color will be seen in the flask. When the lightest pink possible remains in the solution for more than 30 seconds titration is complete. The final volume is recorded, and the same steps are taken for the other two sets of KHP solution. Finally, blank titration is completed to determine deviation.
The k value in run 7 is 75% of that in run 5. This will be directly related to the addition of KNO3 in run 5 and H2O in run 7. These will make different ionic concentrations, resulting in the change in rate constant
A linear formula idea will be used and the decision variables will be labeled as follow:
Table 2 shows the concentrations of S2O8-2 and I- and the time of each reaction for each run. Rate of the reaction was calculated by dividing 1M with the time it took to complete the reaction. The constant k was calculated using the rate law (4), the x and y value was determined by the graphs below. Considering most of the k’s calculated by our laboratory class, the supposed real value of k must be 10/Ms for that reaction.