2. A mass balance is being made for a proposed carbothermic reduction process for thezinc calcine. Enough carbon (in the form of graphite, pure C) will be added to reduceall the lead, zinc oxide and sulphate in the calcine to metallic lead and zinc vapour, andto reduce all the hematite to FeO. The sulphur will leave the system as SO2 and it isassumed that all the carbon will wind up as CO in the off-gas.stoichiometrically required mass of graphite?480 T per day Zinc calcine(72.67% ZnO. 0.25% ZnSO4.17% Fe2O3, 2.37% PbSO4)GraphiteWhat is theZnCarbothermicReduction8Pb FeO SO₂ CO

ZnO+C→Zn+CO ZnSO4+2C→SO2+2CO Fe2O3+C→2FeO+CO PbSO4+2C→Pb+SO2+2CO…

Answered: 2. A mass balance is being made for a…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 9RQ: What characterizes an electrolytic cell? What is an ampere? When the current applied to an...

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When magnesium metal is added to a beaker of HCl(aq), a gas is produced. Knowing that magnesium is oxidized and that hydrogen is reduced, write the balanced equation for the reaction. How many electrons are transferred in the balanced equation? What quantity of useful work can be obtained when Mg is added directly to the beaker of HCl? How can you harness this reaction to do useful work?
The amount of manganese in steel is determined by changing it to permanganate ion. The steel is first dissolved in nitric acid, producing Mn2+ ions. These ions are then oxidized to the deeply colored MnO4 ions by periodate ion (IO4) in acid solution. a. Complete and balance an equation describing each of the above reactions. b. Calculate and G at 25C for each reaction.
Determine the standard free energy change, Gf, for the formation of S2-(aq) given that the Gf for. Ag*(aq) and Ag2S(s) are 77.1 kJ/mole and 395 kJ/mole respectively, and the solubility product for Ag2S(s) is 81051.
When jump-starting a car with a dead battery, the ground jumper should be attached to a remote part of the engine block. Why?
During bad storage of cement the alkalis in the cement react with CO2 to form alkali carbonates, which they react with Ca(OH)2 liberated by the hydrolysis of to form C3S, CaCO3 Calcium Carbonate, C3S Dicalcium silicate, CaCO3 Tricalcium silicate, Calcium Carbonate
A sulfuric acid plant produces a considerable amount ofheat. This heat is used to generate electricity, which helpsreduce operating costs. The synthesis of H2SO4 consists ofthree main chemical processes: (a) oxidation of S to SO2,(b) oxidation of SO2 to SO3, (c) the dissolving of SO3 inH2SO4 and the subsequent reaction with water to formH2SO4. If the third process produces 130 kJ/mol, howmuch heat is produced in preparing a mole of H2SO4 froma mole of S? How much heat is produced in preparing5000 pounds of H2SO4?
A magnesium bar with a mass of 6.0 kg is attached to a buried iron pipe to serve as a sacrificial anode. An averagecurrent of 0.020 A flows between the bar and the pipe.(a) Which reactions take place at the surface of the magnesium bar and the surface of the iron pipe? (b) How many years would it take for the entire magnesium bar to be consumed?
Research has been conducted on molybdates as replacements for chromates in the surface treatment of various metals in order to reduce corrosion by the formation of a surface film of MoO,. The overall reaction with iron is 2Fe(s) + 3M00- (aq) + 6H*(aq) - Fe;Os(s) + 3M0O:(s) + 3H;O() Given the following AG; in calories per mole at 25°C: Fe,O; (s) =-177,100, MoO:(s) =-120,000, H:O (1) =-56,690, Mo0; (aq) =-205,420 (a) Is the above overall reaction spontaneous under standard conditions? (b) Calculate the standard electrode potential for the above overall reaction. (c) Write an expression for the electrode potential as a function of molybdate ion concentration and pH. (d) Is the overall reaction spontaneous for a molybdate ion concentration of 0.001M at pH 7.0?
In the production of magnesium, Mg(OH)2 is precipitatedby using Ca(OH)2, which itself is “insoluble.” (a) Use Ksp valuesto show that Mg(OH)2 can be precipitated from seawater inwhich [Mg2+] is initially 0.052 M. (b) If the seawater is satu-rated with Ca(OH)2, what fraction of the Mg2+is precipitated?
(a) Write the definition of reduction and oxidation. (b) Ammonia oxidizing bacteria (AOB) play an important role in nitrogen cycle. They are also utilized in engineered systems to remove ammonia in wastewater treatment. They obtain energy by oxidizing ammonia NH3 into nitrite (NO2-) and reducing oxygen to water. Balance the reduction and oxidation reactions driven by AOB. (c) Combine the redox reactions into a single reaction. (d) Find ΔG° for the combined reaction. (e) Find ΔG for the given conditions: [NH3] = 2.7 × 10-3 M; pO2 = 0.21 atm; [NO2-] = 1.2 × 10-5 M. If necessary assumeneutral pH (i.e., pH = 7). Are the given conditions favourable for AOB growth?
How many coulombs are released when H2O is oxidized to liberate 1.00 mol O2 in the reaction 2H2O S O2 1 4H1 1 4e2?
8:51 AM Mon Dec 5 = S BIOL 286 E B Lecture Pow... Bb Lecture Pow... O ELECTROCHEMISTRY Recognizing consistency among equilibrium constant, free... cell A B A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG. The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. C Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. n 1 AA 1 1 Explanation 142. kJ/mol O calculated quantities (Check the box next to any that are wrong.) AG - 50. kJ/mol O - 46. kJ/mol O Check www-awu.aleks.com K 24 7.54 x 10 O…

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