Diels-Alder Reaction
Objective: The objective of this lab was to do a diels-alder reaction using anthracene, maleic anhydride, and xylene to create 9,10-dihydroanthracene, 10-, -succinic acid anhydride.
Experimental: Anthracene (1.00g, 5.61x 10-3 mol), maleic anhydride (0.75g, 7.61x 10-3 mol), xylene (5mL, 4.71x 10-2 mol), and a stir rod were added into a round-bottomed flask. The round-bottom flask was then moved to the hood where the it was attached to a distillation column, placed on top of a sand bath. The sand bath temperature was placed between 30C to 40C. At the initial sight of reflux, a timer was set for 40 minutes. The mixture’s appearance was initially green, but darken over time as the experiment proceeded. After 40 minutes, the distillation column was disconnected from the round-bottomed flask. The flask was left alone for 10 minutes to cool back down to room temperature and then placed in an ice bath to crystallize for 10 more minutes. A vacuum filtration was used to collect the crystal onto the Hirsch funnel and a cold xylene flushed the remaining product out of the round-bottom flask. To remove excess fluids from the crystal, filter papers were used to dry the product. The product’s appearance at the end looked similar to a charcoal black color. After the product was dried, it was then weigh out (1.65g). A slow ramp was …show more content…
Theoretical Yield = Theoretical moles x Molecular weight of product (g/mol) Example: Theoretical Yield = 0.00597 (mol) x 276.29 (g/mol)= 1.65 g 3. % Yield= (Actual Yield (g)/ Theoretical Yield (g)) x 100 Example: % Yield = (1.65 (g)/ 1.65 (g)) x 100= 100% 4. Rf value = Distance spot traveled (cm) / Distance solvent traveled (cm)
Example: Rf value = 1.3 (cm) / 4 (cm) = 0.325 cm
Objective: The objective of this lab was to do a diels-alder reaction using anthracene, maleic anhydride, and xylene to create 9,10-dihydroanthracene, 10-, -succinic acid anhydride.
Experimental: Anthracene (1.00g, 5.61x 10-3 mol), maleic anhydride (0.75g, 7.61x 10-3 mol), xylene (5mL, 4.71x 10-2 mol), and a stir rod were added into a round-bottomed flask. The round-bottom flask was then moved to the hood where the it was attached to a distillation column, placed on top of a sand bath. The sand bath temperature was placed between 30C to 40C. At the initial sight of reflux, a timer was set for 40 minutes. The mixture’s appearance was initially green, but darken over time as the experiment proceeded. After 40 minutes, the distillation column was disconnected from the round-bottomed flask. The flask was left alone for 10 minutes to cool back down to room temperature and then placed in an ice bath to crystallize for 10 more minutes. A vacuum filtration was used to collect the crystal onto the Hirsch funnel and a cold xylene flushed the remaining product out of the round-bottom flask. To remove excess fluids from the crystal, filter papers were used to dry the product. The product’s appearance at the end looked similar to a charcoal black color. After the product was dried, it was then weigh out (1.65g). A slow ramp was …show more content…
Theoretical Yield = Theoretical moles x Molecular weight of product (g/mol) Example: Theoretical Yield = 0.00597 (mol) x 276.29 (g/mol)= 1.65 g 3. % Yield= (Actual Yield (g)/ Theoretical Yield (g)) x 100 Example: % Yield = (1.65 (g)/ 1.65 (g)) x 100= 100% 4. Rf value = Distance spot traveled (cm) / Distance solvent traveled (cm)
Example: Rf value = 1.3 (cm) / 4 (cm) = 0.325 cm