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 initial amount final amount A 6.0 g 0g 9.5 g 6.8 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 51.%. Calculate the actual amount of C that was isolated at the end of the reaction. Round your answer to the nearest 0.1 g.

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

2. Ethyl chloride is prepared by the reaction of chlorine with ethane according to the following equation: C:Ho(g) + Cl2(g) – CH$CI(g) + HCl(g) Ethane Ethyl chloride a) Write the balanced chemical equation. Show proof of completion. b) When 5.6 g of ethane is reacted with excess chlorine, determine its theoretical yield c) Calculate the percent yield of ethyl chloride if experimental results indicated that 8.54 g of ethyl chloride had formed.

If the theoretical yield of a reaction is 22.6 gg and the actual yield is 19.9 gg , what is the percent yield?         Express your answer to three significant figures.

Sodium nitrate, manganese (II) sulfate, potassium sulfate, and water is formed from the reaction of sodium nitrite, potassium permanganate, and sulfuric acid. Calculate the actual yield if a percentage yield of 33.01% of sodium nitrate is formed from 47.22 g sodium nitrite, 38.84 g potassium permanganate, and 42.88 g sulfuric acid. Atomic Mass: Na: 22.990 g/mol N: 14.007 g/mol O: 15.999 g/mol Mn: 54.938 g/mol H: 1.008 g/mol S: 32.065 g/mol K: 39.098 g/mol

If 2S02 + 02 -------> 2S03 uses 3.65 g of molecular oxygen and 4.60 g of sulfur dioxide, calculate the maximum amount of sulfur trioxide that can be produced in moles.