The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of19th century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts toform alumina (Al2O3) and water:->>2Al(OH)3(s) Al2O3(s) + 3 H₂O(g)In the second step, alumina (Al2O3) and carbon react to form aluminum and carbon dioxide:2A1,0,(x) + 3C(s) 4Al(s) + 3 CO, (g)->Suppose the yield of the first step is 78.% and the yield of the second step is 97.%. Calculate the mass of aluminum hydroxide required to make 5.0 kg ofaluminum.Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.☐olo□□§4?olo&

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Answered: The extraction of aluminum metal from…

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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There are two steps in the extraction of copper metal from chalcocite, a copper ore. In the first step, copper(I) sulfide and oxygen react to form copper(I) oxide and sulfur dioxide: 2Cu,S(s) 30,(8) 2Cu,0(s) + 2 SO, (g) In the second step, copper(I) oxide and carbon react to form copper and carbon monoxide: Cu,O(s) + C(s) 2Cu(s) + Co (g) Suppose the yield of the first step is 84.% and the yield of the second step is 95.%. Calculate the mass of copper(I) sulfide required to make 4.0 kg of copper. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.
Alum is a compound used in a variety of applications including cosmetics, water purification, and as a food additive. It can be synthesized from aluminum metal, sulfuric acid, water, and potassium hydroxide, as seen in the following equation. Using the data below, determine the theoretical and percent yield for this alumn synthesis. Note that aluminum is the limiting teactant. 2 Al(s) + 2 KOH(aq) + 4 H, SO̟(aq) + 10 H,O(1) → 2 KAI(SO,), · 12 H,0(s) + 3 H,(g) Mass Trial Data Bottle mass (g) 10.1604 Bottle with aluminum pieces (g) 10.2989 Final product and bottle mass (gj 12.492 1 4 PAGES DEC 280 3D F10 F9 F8 F7 F6
Up [References] Ethanol, the alcohol used in automobile fuels, is produced by the fermentation of sugars present in plants. Corn is often used as the sugar source. The following equation represents the fermentation of glucose, the sugar in corn, by yeast to produce ethanol and carbon dioxide. C6 H12 O6 (aq) → → 2C2H; OH(aq) + 2CO2 (g) Ethanol is combusted in an automobile engine according to the equation C2H; OH(1) + 302(g) → 2CO2 (g) + 3H2O(g) What would be the total volume of CO2 gas formed at STP when 4.45 kg of sugar is fermented and the ethanol is then combusted in an automobile engine? Volume = L Submit Answer Try Another Version 3 item attempts remaining
Lead (Pb) has been used for centuries. The Romans used it in their plumbing systems - the symbol for lead (Pb plumbus). To extract the metal, lead (II) sulfide (mineral galena) is roasted in air to form lead (II) oxide (PbO): 2 PbS(s) + 3 O2(g) → 2 PbO(s) + 2 SO2(g) AHrxn = -827.4 kJ Then the lead (II) oxide is reduced with carbon to the metal lead: PbO(s) + C(s) Pb(s) + СО (9) AHrxn = +106.8 kJ a) Use the equations above and Hess's Law to determine the enthalpy of change for the following reaction: PbS(s) + /2 O2(g) + C(s) → Pb(s) + CO (g) SO2(g) ΔΗη [ Select ] kJ (1 mol PbS) b) How much energy (kJ) absorbed (+AHxn) or evolved (-AHpxn) when 400.0 grams of lead (II) sulfide (PbS(s) is converted to lead (Pb)? ΔΗΡη [ Select ] kJ / 400.0 g PbS
Consider the reaction involving the burning of sulfur: 2S(s) + 3O2(g) ->> 2SO3(g) delta Hrxn= ? ? ?
9 a Carbon dioxide is removed from the atmosphere of space capsules by reaction with a solid metal hydroxide. The products are water and the metal carbonate. (a) Calculate the mass of CO₂ that can be removed by reaction with 3.39 kg of lithium hydroxide. x 10 g CO₂ (b) How many grams of CO₂ can be removed by 0.35 kg of each of the following: lithium hydroxide, magnesium hydroxide, and aluminum hydroxide? By lithium hydroxide: x 10 g CO₂ By magnesium hydroxide: x 10 g CO₂ By aluminum hydroxide: x 10 g CO2 & 2 3 # 3 e с $ 4 in de % 5 t A y 7 U 8
There are two steps in the usual industrial preparation of acrylic acid, the immediate precursor of several useful plastics. In the first step, calcium carbide and water react to form acetylene and calcium hydroxide: CaC2(s)+2H2O(g)→C2H2(g)+CaOH2(s) In the second step, acetylene, carbon dioxide and water react to form acrylic acid: 6C2H2(g)+3CO2(g)+4H2O(g)→5CH2CHCO2H(g) Write the net chemical equation for the production of acrylic acid from calcium carbide, water and carbon dioxide. Be sure your equation is balanced.
The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of 19th century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina Al2O3 and water: 2Al(OH)3(s) + Al2O3(s) -> 3H2O(g) In the second step, alumina Al2O3 and carbon react to form aluminum and carbon dioxide: 2Al2O3(s) + 3C(s) + 4Al(s) -> 3CO2(g) Suppose the yield of the first step is 74.% and the yield of the second step is 76.% . Calculate the mass of aluminum hydroxide required to make 4.0kg of aluminum. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.
Over coffee and croissants at breakfast one day, your friend Tom (an expert chemist) says this: "Metal sulfides react with strong acids to produce hydrogen sulfide and a salt." Using Tom's statement, and what you already know about chemistry, predict the products of the following reaction. Be sure your chemical equation is balanced! FeS(s) + HNO3(aq) ->
Aqueous iron(II) sulfate (FeSO4) and solid copper are produced by the reaction of solid iron and aqueous copper(II) sulfate (CuSO4). Write a balanced chemical equation for this reaction. □ X Ś
One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate.Suppose an EPA chemist tests a 250.mL sample of groundwater known to be contaminated with cadmium chloride, which would react with silver nitrate solution like this: CdCl2(aq)+2AgNO3(aq)→2AgCl(s)+CdNO32(aq). The chemist adds 51.0mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 8.9mg of silver chloride. Calculate the concentration of cadmium chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits.
1.58g of magnesium hydrogencarbonate was added to a 1.68 mol/L solution of acetic acid, CH3COOH in water (50.0 mL), producing carbon dioxide gas, water and magnesium acetate, Mg(CH3COO)2. a) Write a balanced chemical equation for the reaction. b) What mass of acetic acid is in the aqueous solution? c) Which of the reactants is the limiting reagent? Justify your answer. d) If 1.23 g of magnesium acetate was produced, what is the percentage yield of the reaction? e) What is the theoretical yield (in grams) of carbon dioxide from this reaction? f) The above reaction is performed in a closed 25 L container at 10 °C. Upon completion of the reaction, what will the final pressure of CO2 be inside the container? please answer d, e and f

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