Biodiesel Synthesis from Canola Oil lab report

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Feb 20, 2024

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Biodiesel Synthesis from Canola Oil Name Section 605 Shanelle Suepaul March 29, 2023 Introduction The purpose of this experiment is to produce biodiesel from canola oil to study the effect of transesterification. Transesterification is a reaction that is used to convert triglycerides in oil into usable oil. It does this by a triglyceride reaction with an alcohol in the presence of a strong acid or base, then producing a mixture of fatty acids alkyl esters and glycerol. My hypothesis is that we will produce a chemical reaction that converts the ester into a mixture of esters of the fatty acids and will be have a high percent recovery. Materials  10mL Graduated Cylinder  100mL Graduated Cylinder  Medium Stir Bars  125mL Erlenmeyer Flask  125mL Beaker  125mL Separatory Funnel  50mL Beakers (3)  Hot Plate  Vegetable Oil  Chemicals  Sodium Hydroxide  Methanol Procedures: 1. Add 0.175g of sodium hydroxide to a 125mL Erlenmeyer flask. 2. Pour 10mL of methanol into the flask and begin stirring for 30 minutes, set the flas aside and cover. 3. Measure 50mL of vegetable oil and pour in to a 125mL beaker. 4. Set it on the hot place with a thermometer at 40 degrees Celsius, then add to the Erlenmeyer flask. 5. Stir the mixture for 30 minutes, then pour in to a 125mL separatory funnel. 6. Use three 50mL beaker labelled, top layer, middle layer and bottom layer. 7. Collect the different layers and obtain the mass for all three layers. Data Table 1 - Mass of Layers in Beakers Layers in Beakers Mass (g) Top layer 33.76

Middle layer (mixture) 4.91 Bottom layer 4.33 Results and Calculations Percent yield =(moles of product/moles of reaction)*100 Percent yield of biodiesel synthesis= (moles of biodiesel/ 3 moles of canola oil)*100 =( (mass of top layer (g)/296.6 (g/mol))/ (3*[(50mL *0.91 g/mL)/885.4 g/mol]*100 Percent yield: 73.9% Analysis - Discussion – Conclusion The percent yield was 73.9%, this means most of the mixture was converted into biodiesel. A human error that could have occurred was the alcohol to oil ratio, if either were added too much or too little it could result in a low percent recovery. An environmental error that could have occurred was the temperature of the lab, depending on the temperature it can have a higher percent recovery, it just depends on the optimal temperature for biodiesel production. Biodiesel is an important source of renewable non-fossil energy that can be used for vehicle engines, it’s being used so petroleum-based fuels, don’t have to be used as much. Post-Lab Questions 2. Why didn’t the two layers separate immediately? The two layers did not separate immediately because the 2 layers including methyl oleate and glycerol have close density values (glycerol-1.26g/mL, methyl oleate-0.87g/mL), thus it takes more time for them to react and then separate from each other. Also, it is because the biodiesel molecule has a polar component. 3. At what point in the reaction is the catalyst reformed? What layer does it end up when the reaction is completed? Sodium hydroxide is a catalyst in this reaction, and it will reform once the reaction is complete. It will end up in the middle layer in the separatory funnel when the reaction is complete. 4. Draw the major biodiesel product that would occur from using palm oil, which is high in triglyceride esters of palmitic acid.

5. What was your percent yield of biodiesel? How might the yield be greater or smaller in industrial production? The percent yield was 73.9%, which is good and means it was converted to biodiesel. The yield would depend on various factors like, temperature, reaction time and alcohol to oil ratio. A higher temperature would produce a greater yield than at a lower temperature.

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Reference Pandey, M; Hoare, A; Weldegirma, A. Practical Chemistry: An Organic Chemistry I Lab Manual , USF St. Petersburg, 2023; pp 85-90 https://pubs.acs.org/doi/10.1021/ie049157g

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