MPT ALLOWED Iron oxide ores, commonly a mixture of FeO and Fe₂O3, are given the general formula FesO4. They yield elemental iron when heated to a very high temperature with either carbon monoxide or elemental hydrogen. Balance the following equations for these processes: Fe3O4 (8) + H₂(g) → Fe(s) + H₂O(g) Fes 04 (8) + CO(g) → Fe(s) + CO₂(g) (Use the lowest possible coefficients for all reactions.) Fe(s) + H₂(g) CO(g)->> Fe(s) + Fe3O4 (8) + Fe3O4 (8) + Submit Answer Try Another Version H₂O(g) CO₂(g) [References] 1 item attempt remaining

MPT ALLOWED Iron oxide ores, commonly a mixture of FeO and Fe₂O3, are given the general formula FesO4. They yield elemental iron when heated to a very high temperature with either carbon monoxide or elemental hydrogen. Balance the following equations for these processes: Fe3O4 (8) + H₂(g) → Fe(s) + H₂O(g) Fes 04 (8) + CO(g) → Fe(s) + CO₂(g) (Use the lowest possible coefficients for all reactions.) Fe(s) + H₂(g) CO(g)->> Fe(s) + Fe3O4 (8) + Fe3O4 (8) + Submit Answer Try Another Version H₂O(g) CO₂(g) [References] 1 item attempt remaining

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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One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CUSO 4(aq) Cu(s) + FeSO4(aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 450. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 147. mg. Calculate the original concentration of copper(II) sulfate in the sample. Round your answer to 3 significant digits. ?
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.
Solid copper can be produced by passing gaseous ammonia over solid copper (II) oxide at high temperatures, according to the following reaction. NH3 (g) + CuO (s) → N2 (g) + Cu (s) + H2O (g) Balance the reaction.
When heated, metal hydroxides decompose to produce a metal oxide and water. Selected the correct balanced equation for the decomposition of calcium hydroxide. CaOH (s) → CaO2 (s) + H2O (g) Ca(OH)2 (s) → CaO (s) + H2O (g) 2 CaOH (s) → 2 CaO (s) + H2O (g) 3 Ca(OH)2 (s) → 3 CaO2 (s) + H2O (g)
Cryolite (Na3AlF6) is used in the commercial production of aluminum from ore. Cryolite itself is produced by the following reaction: 6 NaOH + Al₂O3 + 12 HF → 2 Na3AlF6 + 9 H₂O A mixture containing 420.0 kg of NaOH, 228.4 kg of Al2O3, and 600.0 kg of HF is heated to 950 °C until it reacts to completion. What is the maximum mass of Na3AlF6 formed? kg Na3AlF6
Balance the following chemical equation (if necessary): C₃H₆(g)+O₂(g)→CO₂(g)+H₂O(g)
9. One step in the isolation of pure rhodium metal (Rh) is the precipitation of rhodium(III) hydroxide from a solution containing rhodium(III) sulfate according to the following chemical equation: (Be sure to balance the reaction equation) Rh₂(SO4)3(aq) + NaOH(aq) - Rh(OH)³(s) + Na₂SO4(aq) If 69.28 g of rhodium(III) hydroxide is to be produced, what mass of rhodium(III) sulfate will be needed for the reaction?
Ammonia (NH3) is naturally produced through the decomposition of organic material as wellas being high in wastewater discharged to natural waters. In the environment it is oxidizedto form nitrite (NO2-), and nitrite is then oxidized to form nitrate (NO3-) in a process callednitrification. The balanced equations are given below:2NH3 + 3O2 → 2NO2- + 2H+ + 2H202NO2- + O2 → 2NO3-a) Assuming complete oxidation, what is the theoretical oxygen demand to convert100mg/L of ammonia to nitrate (i.e., how much oxygen is necessary)? Report youranswer as mg/L of O2.Answer: 376 mg/L O2b) This conversion process makes water more acidic. With reference to the equations forpH, explain why this occurs
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6) Consider the following reaction:4NH3 + 50, → 4NO + 6H2O The element being oxidized and the oxidizing agent are: (a)H and NH; (b) O and NH; (c)O and O2 (d) N and O2 (e)N and NH3
Cryolite (Na3AlF6) is used in the commercial production of aluminum from ore. Cryolite itself is produced by the following reaction: 6 NaOH + Al2O3 + 12 HF → 2 Na3AlF6 + 9 H2O A mixture containing 420.0 kg of NaOH, 128.4 kg of Al2O3, and 600.0 kg of HF is heated to 950 °C until it reacts to completion. What is the maximum mass of Na3AlF6 formed? ________kg Na3AlF6
2H2 + 02 (g) → 2 H2O (g) is Decomposition Reactions true False