1. Franklin College plans to use spent cooking oil from the university cafeteria

Question

1. Franklin College plans to use spent cooking oil from the university cafeteria to power all lawn equipment on campus, after it is converted to bio-diesel fuel. The chemistry department receives roughly 160 gallons ofoil every other month. Calculate an approximate amount of methanol (d 0.792 gmL) and NaOH they would need if those two reagents were added at a 3:1 molar amount to each triglyceride. Use the triglyceride below as your hypothetical starting material from the cafeteria. Remember, ! gallon -3.78 L. Approximate density of any cooking oil may be used for this calculation. (9Z9 Z-propane-1,23-tryl trioleate (oleic acid triglyceride) 3 Molecular Weight: 885.43 21

Explanation / Answer

Molar mass of triglyceride = 885.43 g/mol

Density = 0.92 g/mL

Volume of oil = 160 gallons = 160 x 3.78 L = 604.8 x 103 mL

Mass of oil = Volume x density = 604.8 x 0.92 = 5.56416 x 103 g

Number of moles of oil = Mass/MW = 5.56416 x 103/885.43 = 628.41 moles

Number of moles of Methanol = 3 x moles of oil = 3 x 628.41 = 1885.23 moles

Mass of methnol = moles x molar mass = 1885.23 x 32.04 = 60402.7692 g = 60402.7692 /0.792 = 76266.123 mL = 76.266 L

Moles of NaOH = moles of oil = 628.41

Mass of NaOH = moles x molar mass = 628.41 x 40 = 25136.4 g = 25.1364 Kg

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