Calculate the theoretical yield (in grams) of 4-methylcyclohexene expected in this reaction assuming you begin with...
Given the amounts of reactants, please calculate the theoretical yield of the expected alkene reaction product, in mL. Do not factor the sulfuric acid into your calculations. Your final answer must appear in the box provided, or it will not be counted. 4-methylcyclohexanol ------H2SO4(aq) -----> 4-methylcyclohexene Molecular Weight (grams/mole) 114.2 g/mol 98.08 g/mol 96.2 g/mol density (grams/mL) 0.914 g/mL 0.799 g/mL volume (mL) 28.0 mL mass (grams) moles Theoretical yield in mL=
calculate the theoretical yield of the cyclohexenes products in both miles and grams Dehydration of Alcohols Dehydration of 2-Methylcyclohexanol Prelaboratory Mole Calculations Calculate the theoretical yield of the cyclohexer of the starting alcohol gives one mole the mixture of isomers. toles and grams. One mole sing 1.0 mL of 2-methylcyclohexanol and 0.5 mL of the catalyst, H3PO4. NO calculation is needed for the catalyst. OH Н,РО, Third product CH12 one double bond + H2O heat 2-methylcyclohexanol bp 165-168°C d=0.93 g/mL...
What is the theoretical yield calculation of deydration reaction of 4-methylcyclohexanol starting with 7.5 mL to produce 4-methylcyclohexene. Explain steps.
Dehydration of Alcohols Dehydration of 2-Methylcyclohexanol Prelaboratory Mole Calculations Calculate the theoretical yield of the cyclohexenes products in both moles and grams. One mole of the starting alcohol gives one mole the mixture of isomers. You are using 1.0 mL of 2-methylcyclohexanol and 0.5 mL of the catalyst, H3PO4. No calculation is needed for the catalyst. CHE CH3 CH3 OH Н,РО, Third product CH2 + one double bond H2O heat 2-methylcyclohexanol bp 165-168°C d=0.93 g/mL 1-methylcyclohexene bp 110°C 3-methylcyclohexene bp...
Calculate the percent yield of your product assuming you started with 0.545 grams of Al metal and collect 5.25 grams of alum product? 1) Calculate the number of moles of Al used in your reaction. 2) Calculate the molar mass of alum, potassium aluminum sulfate dodecahydrate (do not forget to include the associated water in you molar mass calculation). 3) This experiment has been set up such that Al is the limiting reagent,(determines the maximum amount of product that could...
Chem 143 - Lab 46) CALCULATE THE THEORETICAL YIELD Grams of sodium carbonate used Moles of sodium carbonate used Grams of calcium chloride used Moles of calcium chloride used Moles of precipitate expected Theoretical yield of precipitate in grams Actual yield of precipitate in grams Percent yield 5.6 Show detailed work for percent yield. Page 4 of 4 Chem 143 - Lab Pre-lab Exercise Show the details of each calculation to get full credit 1. Magnesium oxide, a white powdery...
1. What is the theoretical yield of silver chloride (AgCl) if you begin the reaction with 0.2593 g of NaCl? AgNO3(aq)+NaCl(s)---->AgCl(s)+NaNO3(aq) 2. Based on your above calculated theoretical yield, what is the percent yield of AgCl if you produce 0.4829 g experimentally?
Assuming that your reaction has produced only isoborneol, calculate the theoretical yield and percent yield for isoborneol product. Given the mass of isoborneol isolated is 0.184 g. Write appropriate chemical equations, formulas and show all stoichiometric calculations with the mass of pure camphor 0.234g
4. Calculate the theoretical yield of product in the nitration of methyl benzoate if the reaction was begun with 0.400 g of methyl benzoate. (Show ALL work please.)
4.7 Reaction Yields Calculate theoretical yield and percent yield of a reaction given masses of reactants and products Question If the theoretical yield of a reaction is 100 grams, which value for actual yield is physically impossible? Select the correct answer below: O O grams O 50 grams O 99.9 grams 110 grams