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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Similar questions

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%.
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
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 conducts an expirement of the combustion of ethane in the presence of oxygen. The graph below represents data collected in the lab. Which line on the graph above would represent the limiting reactant and which line on the graph above would represent the excess reactant for the combustion of ethane? In your answer, cite specific evidence from the graph to support your determination.
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
Use Factor Method in solving the problems: Step 1. Using the following equation, determine the factor that defines the multiple or the decimal fraction of the amount of formula to be prepared: Quantity of formula desired/Quantity of formula given = Factor A factor greater than 1 represents the multiple of the formula, and a factor less than 1 indicates the fraction of the formula to be prepared. Step 2. Multiply the quantity of each ingredient in the formula by the factor to determine the amount of each ingredient required in the reduced or enlarged formula. 1. From the following formula, calculate the quantity of each ingredient required to make 1 gallon of compound benzoin tincture. Benzoin 100 g ? Aloe 20 g ? Storax 80 g ? Tolu balsam 40 g ? Alcohol, to make 1000 mL 1 gallon 1 gallon = 3785 mL *Note: Give your final answer in 2 decimal places. Indicate the unit.
Why it's impossible to get a hundred percent yield from the original sample?
answer the following mole question
An unknown compound is 40.0% C, 6.7% H, and 53.3% O by mass, and has a molecular molar mass of 120 g/mol. Create a step-by-step list of how you could determine the molecular formula. Within your written process, provide answers to include units and provide the correct molecular formula.
A compound containing only carbon, hydrogen, and oxygen is analyzed using combustion analysis. When 80.9 g of the compound is burned, 148.2 g of carbon dioxide and 40.5 g of water are collected. 1.) In order to determine the moles of carbon in the compound, first determine the moles of carbon dioxide that were produced from the combustion. 2.) Determine the moles of carbon present in carbon dioxide. This will be the same number of moles of carbon in the original compound. 3.) In order to determine the moles of hydrogen in the compound, first determine the moles of water that were produced from the combustion. 4.) Determine the moles of hydrogen present in the water. This will be the same number of moles of hydrogen in the original compound. 5.) Calculate the mass of oxygen in the original compound. You will need to subtract the mass of the carbon that ended up in the carbon dioxide and the mass of the hydrogen that ended up in the water from the mass of the original compound. 6.)…
DUE NOW. Please answer it with the correct significant figures. Thank you!

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