ChE 311: Industrial Chemistry

INTRODUCTIONIndustrial Chemistry deals with the preparation of products from raw materials through the agency of chemical change.Chemistry is important to industry by: Regulating manufacturing process Quality Control Research & DevelopmentSources of Raw Materials from the natural environment Lithosphere Earths Crust Hydrosphere Marine and Oceanic Environment Atmosphere Air Plants FloraClassification of Natural Resources1. Renewable Resources that generate themselves Forestry, fishery, and wildlife2. Non-Renewable Resources that are formed over long periods of time Minerals, metals, and organic materials Renewable resources can be non renewable when the rate of consumption of renewable resources is greater than the rate of regenerationChemical Industries commonly manufactured: Heavy Chemicals Common acids, soda ash, salt Fine Chemicals Result from a series of small-scale chemical operationsCharacteristics of Chemical Industry It must be essentially science-based industry It must be with great commitment and investment to Research & DevelopmentEight Standard Industrial Classifications1. Industrial Inorganic Chemicals2. Plastic Materials, and Synthetics3. Drugs4. Soap, Cleaners, and Toilet Goods5. Paints and Allied Products6. Industrial Organic Chemicals7. Agricultural Chemicals8. Miscellaneous Chemical Products

Typical Structure of a Chemical Manufacturing ProcessRaw MaterialsSeparation & PurificationsChemical ReactionsPhysical TreatmentRaw Materials

Unreacted Materials

Primary Types of Chemical Reactions1. Batch Reactions-Chemicals are added to the reactor at the same time and products are emptied completely when the reaction is finished2. Continuous Reactions-Reactants are added and products are removed at a constant rate from the reactor

General Principles of Industrial Chemistry- When undertaking a case study of a particular chemical industry, the following characteristics must be studied:1. Feedstock (Raw materials, preparation)2. Rate(Temperature and Pressure Variables)3. Production Yield4. Co-Products/By-Products5. Waste Disposal and Effluent Control6. Quality Control7. Safety8. Costs9. Site Location10. Suitable Materials for the Construction of a Chemical Plant

Stoichiometric Relations

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Problems for Stoichiometry1. The most important commercial process for converting N2 from the air into nitrogen-containing compounds is based if the reaction of N2 and H2 to form ammonia (NH3). a) How many moles of NH3 can be formed from .1071 gram of N2 and 3 grams of H2?b) Which is the Limiting Reactant?c) Which is the Excess Reactant?2. A strip of zinc metal with a mass of 2.00 g is placed in an aqueous solution containing 2.50g of silver nitrate, causing the following reaction to occur:Zn (s) + 2 AgNO3 (aq) 2 Ag (s) + Zn(NO3)2 (aq)a) Which is the limiting reactant? b) How many grams of Ag will form?c) How many grams of Zn(NO3)2 will form?d) How many grams of excess reactant will be left at the end of the reaction?3. Adipic Acid, H2C6H8O4, is used to produce nylon. The acid is made commercially by a controlled reaction between cyclohexane (C6H12) and O2:2 C6H12 (l) + 5 O2 (g) 2 H2C6H8O4 (l) + 2 H2O (g)a) Assume that you carry out this reaction starting with 25.0 g of cyclohexane and that cyclohexane is the limiting reactant. What is the theoretical yield of adipic acid?b) If you obtain 33.5 g of adipic acid from your reaction, what is the percentage yield of adipic acid?4. In a small scale reaction, the process by which iron ore containing Fe2O3 is converted into iron by the equation:Fe2O3 (s) + 3 CO (g) 2 Fe (s) + 3 CO2 (g)a) If you start with 150 g of Fe2O3 as the limiting reagent, what is the theoretical yield of Fe?b) If the actual yield of Fe in your test was 87.9 g, what was the percentage yield?5. Antimony is obtained by heating pulverized stibnite (Sb2S3) with scrap iron and drawing off the molten antimony from the bottom of the reaction vessel:Sb2S3 + Fe Sb + FeSSuppose that 0.600 kg of stibnite and 0.250 kg of iron turnings are heated together to give 0.200 kg of Sb metal.Calculate the following:a) Limiting Reactantb) Percent Excess Reactantc) Degree of Completiond) % Conversion of Sb2S3 to Sbe) Yield of Sb

Problems for Gas Laws1. A sample of 100 grams of an ideal gas at 0.8 bar pressure has its volume doubled and absolute temperature tripled. Find the final pressure.

2. Calcium Carbonate, CaCO3(s), decomposes upon heating to give CaO(s) and CO2(g). A sample of CaCO3 is decomposed, and the carbon dioxide is collected in a 250-ml flask. After the decomposition is complete, the gas has a pressure of 1.3 atm at a temperature of 31oC. How many moles of CO2 gas were generated?

3. Find the molar volume of an ideal gas at 23oC and 1atm.

4. What is the density of N2 at 80oC and 745 mmHg compared to air at 80oC and 745 mmHg?

5. A certain mixture of N2 and O2 has a density of 1.185g/L at 101.325kPa. Find the mole fraction of O2 in the mixture.

6. A gaseous mixture made from 6.00g O2 and 9.00g CH4 is placed in a 15.0L vessel at 0oC. What is the partial pressure of each gas, and what is the total pressure in the vessel?

7. A study of the effects of certain gas on plant growth requires a synthetic atmosphere composed of 1.5 mol percent CO2, 18.0 mol percent O2, and 80.5 mol percent Ar.a. Calculate the partial pressure of O2 in the mixture if the total pressure of the atmosphere is to be 745 torr.b. If this atmosphere is to be held in a 121-L space at 295K, how many moles of O2 are needed?

8. A sample of KClO3 is partially decomposed, producing O2 gas that is collected over water. The volume of gas collected is 0.250-L at 26oC and 765 torr total pressure.a. How many moles of O2 are collected?b. How many grams of KClO3 were decomposed?Prepared by: Benedict S. Marzan5