WebApr 10, 2024 · NH 2-BTD (0.152 g, 1.0 mmol) was dissolved in 25 mL of dry dichloromethane and 3 Å molecular sieves (about 3.0) g were added. A stoichiometric amount of freshly distilled pyridine-2-carboxaldehyde (96 μL) was introduced with a microsyringe and the reaction mixture was refluxed for six hours. WebTranscribed image text: After mixing for two hours, the product is extracted into Dichloromethane and the solvent is removed to give 0.3 g of a yellow oil. Question #22: Using the mmoles of Methylcyclopentene calculated earlier and the molecular weight of the product (179 g/mol) predict the theoretical 100% yield of the product in grams.
Chemistry 1 : Exam 4 Flashcards Quizlet
WebMay cause cancer based on animal data. May be harmful if inhaled. May cause irritation of respiratory tract. Inhalation may cause central nervous system effects. WARNING! This product contains a chemical known in the State of California to cause birth defects or. Wear personal protective equipment. Use only under a chemical fume hood. WebApr 14, 2024 · The results of molecular docking showed that compound R8 had a maximum binding affinity for H+/K+ ATPase of –9.3 kcal/mol. The study revealed that compound R8 has a potent activity and can be used as a lead molecule. ... (3 equiv.) in dry dichloromethane at 0°C was added to aryl sulfonyl chlorides (1.2 equiv.). The reaction … cub foods rogers mn weekly ad
Dichloromethane CAS 75-09-2 106454 - Merck Millipore
WebAt a temperature of 20 degrees Celsius the density of dichloromethane is 1.326 g/mL. At a temperature of 25 degrees Celsius the density is 1.317. At a temperature of 90 degrees … WebWhat mass of sucrose (molar mass= 342.30 g/mol) would be needed to dissolve in 500.0 g of water? Kb (water) = 0.512°C/m. E) 130. g sucrose: 64) Determine the boiling point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 722 mL of benzene (d = 0.877 g/mL). Pure benzene has a boiling point of … WebFeb 25, 2024 · We know that 1 mol CH2Cl2 = 84.93 g CH2Cl2 Start with your given quantity and convert it to the energy required to vaporize it by using conversion factors based on these relationships: 48.7 g CH2Cl2 x (1 mol CH2Cl2 / 89.3 g CH2Cl2) x (31.6 kJ / 1 mol CH2Cl2) = 17.2 kJ You should always be able to check to see if the answer makes sense. east cobb family practice