Use the following atomic weights and quantities to calculate the overall % yield of hexaphenylbenzene using the following abstractequation. Assume that all the inorganic reagents are in excess but remember that your yield must be based on the stoichiometry, thelimiting reagent, and that grams must be converted to moles. Filling out most of the chart will help. Give only two significant digits inyour 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 = 313PhPh-FePhPh.CIB122PhH4NO NPhiOHPhiPhPh=C:0FePhPh2 HBrN₂Ph-Ph C5 H₂OPhHC1H₂formulaformula weightbenzaldehyde phenylacetic acid benzyltriphenylphosphonium chloride -> hexaphenylbenzenemilliliters3.84316.754density1.044gramsmolesAnswer:5.9825.592% yield?

i) Volume of benzaldehyde=3.843ml Density of benzaldehyde =1.044g/ml Mass of benzaldehyde =…

Answered: Use the following atomic weights and…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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please put the right number of significant figures
The actual yield of one of the reactions in 43.5g. What was theoretical yield in the laboratory if the scientist concluded that % yield of the reaction ended up to be 77%.
“Magnesium metal is burned in the presence of atmospheric oxygen to form magnesium oxide. Student 1 data Mass Mg 0.1712 g Mass after reaction 0.2886 g Using the given data, calculate the stoichiometric ratio of magnesium ions to oxygen ions in this magnesium oxide sample. Express the ratio as a decimal. Include four significant figures.”
my theoretical yield was 45.0g. If my percent yield was 68.0%, how much was my actual yield?
Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 4.29g of magnesium co ribbon burns with 9.01g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. Incorrect What is the limiting reactant? magnesium oxygen If the percent yield for the reaction is 84.9%, how many grams of product were formed? mass of product formed tneorrect How many grams of the excess reactant remain? mass of excess reactant: g
If the molecules in the above illustration react to form NH3 according to the equationN2 + 3 H2 2 NH3 , the limiting reagent is...
It was determined that 1.4 x 1024 carbon dioxide molecules are produced when propane is combusted according to the equation below. Calculate the number of moles of propane that was burned.
A student prepared benzil according to the experimental procedure using 2.58 g. of benzoin and 12 mL of nitric acid. The mass of the crude benzil product was 2.25 g. and the mass of the recrystallized benzil product was 1.95 g. Find the molecular weights for benzoin and benzil, then answer the following questions. What was the percent yield of the crude benzil? Assume units of %. Round answer to the first decimal place. What was the percent yield of the purified benzil? Assume units of % Round answer to the first decimal place. What was the percent recovery of the purified benzil from the crude benzil? Assume units of % Round answer to the first decimal place.
DDT, which can be prepared by the reaction shown below, was an insecticide used to prevent mosquito borne diseases. Due to the harmful effects on birds and fish, it is now banned in the US. However, other countries still use it to control mosquitos. Determine the amount of DDT that can be produced and the percent yield for this reaction by constructing a BCA table, determining the maximum grams of DDT that can be produced, and calculating the percent yield. Complete Parts 1-3 before submitting your answer. 1 Before (mol) Change (mol) After (mol) 2 C₂H₂CI+ C₂HOCI → C₁H₂Cl + H₂O 3 14 9 5 2 3 NEXT > If a company in South America started with 1175 g of chlorobenzene (CH₂CI, MW 112.55 g/mol) and 538.5 g of chloral (C₂HOCI, MW 147.39 g/mol), set up the table below that represents 100% yield with the given reaction conditions. 2 C₂H₂CI + C₂HOCI CH.CI 14 9 5 + H₂O
Potassium metal reacts with oxygen gas to produce potassium oxide when heated with in air. A chemist starts a reaction with 3 moles of potassium and 5 moles of oxygen gas. What is the theoretical yield in moles of potassium oxide that can be produced? Round to 2 significant digits. If a chemist isolates 1.3 mol of potassium oxide from this reactions what is the % yield for this reaction? Round to 2 significant digits.
Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients. NH₂(g) + O₂(g) + CH₂(g) HCN (aq) + H₂O(1) ローロ X Ś
What is the computation for the theoretical yield of benzoic acid?

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