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. 2 C₂H₂CI+ C₂HOCI - C₁₂H₂Cl₂ + H₂O 1 Before (mol) Change (mol) After (mol) 2 NEXT If a company in South America started with 1175 g of chlorobenzene (CHCI, 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. 3 2 C₂H₂CI + C₂HOCI C₁H₂CI + H₂O

What is the % yield of the reaction? What is the limiting reagent? Show complete calculations for the theoretical and % yield calculations, please. Bromobenzene: 4.5mL Magnesium:1.0g Methyl benzoate:2.5mL

Question 25 of 97 Submit DDT 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. It can be prepared by the reaction shown below. Determine the amount of DDT that can be produced and the percent yield for this reaction. 2C6H,CI + C2HOCI, – C,4H9CI, + H20 2 3 NEXT If a company in South America started with 1175 g of chlorobenzene (C6H5CI, MW 112.55 g/mol) and 538.5 g of chloral (C2HOCI3, MW 147.39 g/mol), set up the table below that represents 100% yield with the given reaction conditions. 2C6H,CI C2HOCI, C1.H,Cls H2O Before (mol) Change (mol) After (mol) O RESET 3.132 -3.132 3.654 -3.654 7.308 0. + -7.308 10.44 -10.44 MacBook Air F12 II F8 F10 F11 000 F9 20 F3 F7 F4 F5 F6 esc F2 F1 +.

An excess of sodium carbonate, Na2CO3, in solution is added to a solution containing 17.87 g CaCl2. After performing the experiment, 12.51 g of calcium carbonate, CaCO3, is produced. Calculate the percent yield of this reaction.

For the following reaction, determine the mass of Sulfur would be needed to obtain 80.0 g of CS2. The percent yield of the reaction is consistently 92%.  CH4 (g) + 4S (g) → CS2 (g) + 2H2S (g)

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.

GIVEN C4H10 (g)    +    O2(g)   →      CO2 (g)   +    H2O (l) - Balance this reaction equation - Calculate the mass of CO2 produced when 10.5 g of C4H10 react with 15.0 g of O2.   - What is the experimental yield if the percent yield in one experiment is found to be 75.5%?

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

Use this table to answer the following questions below: Before reaction Before reaction Theoretical yield Theoretical yield Actual yield Yes, it is balanced. Other: Is the chemical reaction involved balanced? If not, kindly type the correct balanced equation. Please take note that subscripts cannot be written properly. What is the percentage yield in this experiment? * 96.3% 93.6% CH3OH 32.0 g 1.00 mol 36.9% 63.9% CO Excess Excess CH3COOH 0 0 1.00 mol 60.0 g 57.8 g