100 kg of roasted zinc ore with composition: 66% ZnO, 3% ZnS, 10% PbO, 14% Fe203, 1% Al203, 6% SiO2 is reduced in a horizontal retort furnace with 45 kg coke having 90% C and 10% SIO2. In the furnace 91% of ZnO is reduced to Zn 100% of PbO is reduced to Pb 75 % of Fe304 is reduced to Fe, 25 % of Fe3O4 is reduced to FeO Neglect the vaporization of Pb and Fe and accept that they will not reoxidize. 1. Determine the weight of zinc and the percentage of zinc gained from the ore. 2. Determine the theoretical weight of C required for the reduction of Zno and the percentage of the excess C. 3. Determine the weight and the percentage of the residual material in the retort furnace after the removal of zinc vapor.

100 kg of roasted zinc ore with composition: 66% ZnO, 3% ZnS, 10% PbO, 14% Fe203, 1% Al203, 6% SiO2 is reduced in a horizontal retort furnace with 45 kg coke having 90% C and 10% SIO2. In the furnace 91% of ZnO is reduced to Zn 100% of PbO is reduced to Pb 75 % of Fe304 is reduced to Fe, 25 % of Fe3O4 is reduced to FeO Neglect the vaporization of Pb and Fe and accept that they will not reoxidize. 1. Determine the weight of zinc and the percentage of zinc gained from the ore. 2. Determine the theoretical weight of C required for the reduction of Zno and the percentage of the excess C. 3. Determine the weight and the percentage of the residual material in the retort furnace after the removal of zinc vapor.

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter24: Coulometry

Section: Chapter Questions

Problem 24.9QAP

See similar textbooks

Similar questions

A sample of feldspar weighing 1.500g is decomposed, and eventually there is obtained a mixture of KCl and NaCl weighing 0.1801 g. These chlorides are dissolved in H2O, a 50-mL pipetful of 0.08333 N AGNO3 is added, and the precipitate is filtered off. The filtrate requires 16.47 mL of 0.1000N KCNS, with ferric alum as indicator. Calculate the percentage of K2O in the silicate.
Fe2O3 is produced from a pyrite concentrate containing 65% by weight of pyrite (FeS2) by total oxidizing roasting according to the following reaction. 5 tons of pyrite concentrate is roasted daily (MA, g / mol; Fe: 56; S: 32; 0: 16; H: 1). 2FeS2 + 11 / 2O2 → Fe2O3 + 4SO2 How much Fe2O3 is produced in 1 day?
A sample of iron ore weighing 800 mg was treated with HNO3 , boiled to dryness and redissolved in dilute HCl. After filtration and removal of undissolved silica, the liquid was passed through a Walden reductor. The collected sample was titrated with 0.0210 M KMnO4 , requiring 12.0 mL to reach the end point. Calc %Fe (55.845) in the ore.
Pyrite (FeS2) is often roasted to obtain sulfur dioxide for making sulfuric acid. Consider the roasting reactionFeS2 + O2 = Fe2O3 + SO2Stoichiometric exercises:a) Formulate the correct stoichiometric roasting reaction Calculate, in respect to 1 t of pyrite, the stoichiometric amounts ofb) Oxygen required for roasting (in m3) c) Obtained hematite by-product (in t) d) Sulfur dioxide produced (in m3) Thermodynamic considerations:e) Calculate the reaction enthalpy ∆Ho298 for the above roasting reaction (in MJ/t of pyrite) Mind you: Requested is the reaction enthalpy per 1 t of pyrite! f) State whether the reaction is exo- or endothermic and say why. g) Calculate the actual change of entropy ∆So298 in J/(mol K) and explain why it is positive or negative
One can view the blast furnace from a simple viewpoint as a process in which the principal reaction is: Fe2O3 + C → Fe + CO But some other undesirable side reactions occur, mainly Fe2O3 +C → FeO+CO After mixing 600 lb of carbon (coke) with 1.00 ton of pure iron oxide, Fe2O3, the process produces 1200 lb of pure iron, 183 lb of FeO and 85 lb of Fe2O3. Calculate the pounds of carbon used up and the pounds of CO produced per ton of Fe2O3 charged and the selectivity in this process (of Fe with respect to FeO).
An impure sample of Na3PO3 weighing 0.1392 g was dissolved in 25 mL of water. A solution containing 50 mL of 3% w/v mercury(II) chloride, 20 mL of 10% w/v sodium acetate, and 5 mL of glacial acetic acid was then prepared. The solution containing the phosphite was added dropwise to the second solution, oxidizing PO3^3– to PO4^3– and precipitating Hg2Cl2. After digesting, filtering, and rinsing, the precipitated Hg2Cl2 was found to weigh 0.4320 g. Report the purity of the original sample as %w/w Na3PO3. Moles Na3PO3 = moles Hg2Cl2
A sample of an iron ore was prepared for Fe3+ analysis as following: 3.4g of the sample was added anddissolved in acid environment then diluted to 250 mL using volumetric flask. After that, 10 mL of the resultingsolution was transferred by pipet to a 50-mL volumetric flask and continue to be diluted. The scientists foundout that this solution gives the concentration of Fe3+ as 2.3 mg/L. Find the weight percentage of Fe3+ in theoriginal sample.
The chief chemist of the Brite-Metal Electroplating Co. isrequired to certify that the rinse solutions that are discharged from the company’s tin-plating process into the municipal sewer system contain no more than 10 ppm (parts per million) by mass of Sn2+. The chemist devises the following analytical procedure to determine the concentration. At regular intervals, a 100-mL (100-g) sample is withdrawn from the waste stream and acidified to pH = 1.0. A starch solution and 10 mL of 0.10 M potassium iodide are added, and a 25.0-mA current is passed through the solution between platinum electrodes. Iodine appears as a product of electrolysis at the anode when the oxidation of Sn2+ to Sn4+ is practically complete and signals its presence with the deep blue color of a complex formed with starch. What is the maximum duration of electrolysis to the appearance of the blue color that ensures that the concentration of Sn2+does not exceed 10 ppm?
Silver(ag) is obtained in much of the same manner as gold using NaCN solution and O2. Describe with appropriate equation the extraction of Ag from argentite Ag2S. The products are SO2 and Ag(CN)2 which are reduced with ZN?
Given: You weigh out exactly 0.200 g of Fe(NH4)2(SO4)2·6H2O and dissolve it in the 100.00 mL volumetric flask. You then pipette 2.00 mL of this solution into the 50.00 mL volumetric flask to prepare the stock standard tris-bipyridyl-iron(II) solution. a. Calculate the molar concentration of iron(II) in this solution in the 50.00 mL volumetric flask. (The MW of Fe(NH4)2(SO4)2·6H2O is 392.14 g/mol) (answer a given the information above)
Copper is produced from chalcopyrite concentrate from a mixed type ore containing 1.2% CuFeS2 (chalcopyrite) and 6% Cu3 (CO3) 2 (OH) 2 (azurite) by sulfating roasting leaching method. 4 tons of chalcopyrite concentrate is roasted daily. If it is assumed that the amount of iron in the solution is 20% under the same conditions, how much copper is produced in 1 day?
Method of separation/chemical reaction (with the brief process) of 3 KG's OF SODIUM BORATE AND 1.5 KG's HYDROCHLORIC ACID