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 ?

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?