Question5 DDT, an insecticide harmful to fish, birds, and humans, is pre duced by the following reaction: 2C,H,CI + CHOCI, CH,Cl, + H,O chlorobenzene chloral DDT In a government lab, 1142 g of chlorobenzene is reacted wish 485 g of chloral. a. What mass of DDT is formed, assuming 100% yield? b. Which reactant is limiting? Which is in excess? c. What mass of the excess reactant is left over? d. If the actual yield of DDT is 200.0 g, what is the percent yield?
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- Ferrocene, Fe(C5H5)2(s), can be prepared by reacting 3.0 g of FeCl2(s) with anequal mass of cyclopentadiene, C5H6(l), and an excess of KOH, as shown in thefollowing reaction FeCl2 + 2C5H6 + 2KOH → FeC10H10 + 2H2Oa. What is the limiting reagent in this procedure?b. Based on your answer to part A, what mass of Fe(C5H5)2 couldtheoretically be formed?c. A student who carried out this reaction obtained 2.7 g of ferrocene. Whatwas the percent yield for this reaction?Compound A reacts with Compound B to form only one product, Compound C , and it's known the usual percent yield of C in this reaction is 91.% . Suppose 8.0g of A are reacted with excess Compound B, and 8.2g of Compound C are successfully isolated at the end of the reaction. What was the theoretical yield of C ?Round your answer to the nearest 0.1g How much B was consumed by the reaction?The following is the balanced equation for the combustion of butanol in oxygen:C4H9OH(g) + 6O2 --> 4 NO(g) + 6H2O(g) a. How many grams of butanol must be burned to produce 18.50g of carbon dioxide? b. How many grams of water are also produced? c. How many grams of oxygen are needed to produce 18.50g of carbon dioxide? d. Use the results from a, b and c to show this reaction obeys the law of conservation of mass.
- In 1997, at the United Nations Conference on Climate Change, the major industrial nations agreed to expand their re-search efforts to develop renewable sources of carbon-basedfuels. For more than a decade, Brazil has been engaged in aprogram to replace gasoline with ethanol derived from the rootcrop manioc (cassava).(a) Write separate balanced equations for the complete combus-tion of ethanol (C₂H₅OH) and of gasoline (represented by theformula C₈H₁₈).(b) What mass of oxygen is required to burn completely 1.00 Lof a mixture that is 90.0% gasoline (d=0.742 g/mL) and 10.0%ethanol (d=0.789 g/mL) by volume?(c) If 1.00 mol of O₂ occupies 22.4 L, what volume of O₂ isneeded to burn 1.00 L of the mixture?(d) Air is 20.9% O₂ by volume. What volume of air is needed toburn 1.00 L of the mixture?Adipic acid, H2C6H8O4, is used to produce nylon. It is made commercially by a controlled reaction between cyclohexane ( C6H12 ) and O2:. (Only the 4th sub part (d) is needed to be answered). 2 C6H12 (l) + 5 O2 (g) → 2 H2C6H8O4 (l) + 2 H2O (g) (Given: Atomic Wts (g/mol): C= 12.01 ; H=1.01 ; O=16.00 ) If 25.0 g of cyclohexane is reacted with 20.0 g of O2, a. Identify the limiting reactant and excess reactant? b. How much in grams of the excess reactant will be left after the reaction? c. What is the theoretical yield in terms of the product adipic acid? d. If the actual yield is 33.5 g, what is the % yield of adipic acid?Sulfur trioxide dissolves in water to make sulfuric acid, H2SO4. a. Write a balanced chemical equation for the reaction. b. Calculate the mass of sulfuric acid that could be produced from the reaction of 10.0 mL of water (d=00g/mL) and 20.0 g of SO3? c. Yeast converts glucose (C6H12O6) into ethanol (d=789g/mL) in a process called fermentation. An equation for the reaction can be written as follows: i. Balance the equation. ii. If the percent yield of ethanol is only 77.1%, how many grams of glucose must react to make 80.0mL of ethanol?
- 3. Syngas is a mixture of carbon monoxide, carbon dioxide, and water vapor that is used for making fertilizer, methanol, and other products. It is produced by heating fossil fuels under low-oxygen conditions to promote incomplete combustion. Write an equation for the complete combustion of the gasoline component cyclopentane, C5H10 (l) and the incomplete combustion of cyclopentane with 20% of the carbon appearing as CO(g).Given (8.79x10^6) moles of glucose, C6H12O6, calculate the mole of carbon dioxide, CO2, formed upon complete oxidation of the glucose. C6H12O6 + 6 O2 → 6 CO2 + 6 H2O Express your answer in three significant digits as moles. Note: Your answer is assumed to be reduced to the highest power possible.Adipic acid, H2C6H8O4, used to produce nylon, is made commercially by a reaction between cyclohexane 1C6H122 and O2:2 C6H121l2 + 5 O21g2¡2 H2C6H8O41l2 + 2 H2O1g2(a) Assume that you carry out this reaction with 25.0 g of cyclohexane and that cyclohexane is the limiting reactant. What is thetheoretical yield of adipic acid? (b) If you obtain 33.5 g of adipic acid, what is the percent yield for the reaction?
- How many kg of Co2 are produced when 1.00 gallon of octane (C8H18, density = 0.703 g/mL) is completely combusted in the presence of O2 to form CO2 and H2O?Gasoline is composed primarily of hydrocarbons, includingmany with eight carbon atoms, called octanes. One ofthe cleanest–burning octanes is a compound called 2,3,4-trimethylpentane, which has the following structural formula The complete combustion of one mole of this compoundto CO21g2 and H2O1g2 leads to ΔH° = -5064.9 kJ.(a) Write a balanced equation for the combustion of1 mol of C8H181l2. (b) By using the information inthis problem and data in Table 5.3, calculate ΔHf° for2,3,4-trimethylpentane.Given the following balanced reaction, Fe2O3+3C-->2Fe+3CO if 1140 of fe2o3 were reacted with ecess c, what would be the percent yield for the reaction if 455g of CO were actually collected? density fe2o3=5.24g/cm3, density of co is 1.14kg/m3