Use the following atomic weights and quantities to calculate the overall % yield of stilbene dibromide. Remember that your yield must be based on the limiting reagent, and that grams must be converted to moles. Filling out most of the chart will help. Give only two significant digits in your answer. If after rounding the answer is a whole number, do not include a decimal point. C = 12, H = 1, Br = 80, CI = 35.5, N = 14, Na = 23, O = 16 sodium hydroxide water tetrabutylammonium bromide cyclohexene chloroform 7,7-dichlorobicyclo[4.1.0]heptane formula formula weight milliliters 0.848 5.122 3.533 density 1 0.811 1.49 grams 2.795 29.001 6.687 moles % yield ? Answer:

In a certain chemical reaction Compound A combines with Compound B to produce Compound C (and no other products). Measurements were taken of the amounts of A and B present before and after a reaction that produced some C: Compound A B initial amount final amount 7.0 g 0 g 5.0 g 3.4 g Calculate the theoretical yield of C. Round your answer to the nearest 0.1 g. Suppose the percent yield of C in this reaction was 89.%. Calculate the actual amount of C that was isolated at the end of the reaction. Round your answer to the nearest 0.1 g. Explanation Check 0 0 ロ・ロ X 1 00 79 4 S 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use E OL E Privacy Center | Accessibil

how to calculate the molecular formula of 65.45% carbon, 5.45% Hydrogen, 29.09% Oxygen and has a molar mass of 110.0 g/mol

Compound A reacts with Compound B to form only one product, Compound C, and it's known the usual percent yield of C in this reaction is 55.%. Suppose 2.0 g of A are reacted with excess Compound B, and 4.4 g of Compound C are successfully isolated at the end of the reaction. What was the theoretical yield of C? Round your answer to the nearest 0.1 g. How much was consumed by the action? Round your answer to the nearest 0.1 g.

How many moles of Fe2O3Fe2O3 are in 171 g171 g of the compound?

What factors during the reducing bezil experiment caused the percent yield to be different than 100%? What impurities may be present in the final product and how does that effect the percent yield determination?

How many moles of Cl2 are required to produce 9.6 moles of PCl3 by the reaction 2P+3Cl2–>2PCl3

Use the following atomic weights and quantities to calculate the overall % yield of hexaphenylbenzene using the following abstract equation. Assume that all the inorganic reagents are in excess but remember that your yield must be based on the stoichiometry, the limiting reagent, and that grams must be converted to moles. Filling out most of the chart will help. Give only two significant digits in your answer. If after rounding the answer is a whole number, do not include a decimal point. C=12, H = 1, CI = 35.5, O= 16, P = 31 3 Ph Ph- Fe Ph Ph. CI B12 2 Ph H4NO N Phi OH Phi Ph Ph =C: 0 Fe Ph Ph 2 HBr N₂ Ph -Ph C 5 H₂O Ph HC1 H₂ formula formula weight benzaldehyde phenylacetic acid benzyltriphenylphosphonium chloride -> hexaphenylbenzene milliliters 3.843 16.754 density 1.044 grams moles Answer: 5.982 5.592 % yield ?

Please do not round off intermediate calculations. Thank you.

What is the mass of 2.00 mol of chlorotrifluoromethane?     52.1 g     209 g     104 g     418 g     0.0104