Blast furnaces extra pure iron from the iron(III) oxide in iron ore in a two step sequence. In the first step, carbon and oxygen react to form carbon monoxide: 2C(s) + O₂(g) → 2CO (g) In the second step, iron(III) oxide and carbon monoxide react to form iron and carbon dioxide: Fe₂O3(s) + 3C0 (g) 2Fe(s) + 3 CO₂ (g) Suppose the yield of the first step is 60.% and the yield of the second step is 72.%. Calculate the mass of carbon required to make 5.0 kg of iron. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.

Blast furnaces extra pure iron from the iron(III) oxide in iron ore in a two step sequence. In the first step, carbon and oxygen react to form carbon monoxide: 2C(s) + O₂(g) → 2CO (g) In the second step, iron(III) oxide and carbon monoxide react to form iron and carbon dioxide: Fe₂O3(s) + 3C0 (g) 2Fe(s) + 3 CO₂ (g) Suppose the yield of the first step is 60.% and the yield of the second step is 72.%. Calculate the mass of carbon required to make 5.0 kg of iron. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.

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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Blast furnaces extract pure iron from the iron(III) oxide in iron ore in a two step sequence. In the first step, carbon and oxygen react to form carbon monoxide: 2 C(s) + O₂(g) →2 CO(g) In the second step, iron(III) oxide and carbon monoxide react to form iron and carbon dioxide: Fe₂O3(s) + 3 CO(g) →2 Fe(s)+3 CO₂(g) Write the net chemical equation for the production of iron from carbon, oxygen and iron(III) oxide. Be sure your equation is balanced.
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.
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 for the production of NO₂ from NO: 2 NO(g) + O₂ (g) → 2 NO₂ (g)
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
Which of the following is the formation reaction for Na2CO3 (s)? A. 2 Na(s) + C(s, graphite) + 3 O(g) → Na2CO3(s) B. 4 Na(s) + 2 C(s, graphite) + 3 O2(g) → 2 Na2CO3(s) C. 2 Na(s) + C(s, graphite) + 1.5 O2(g) → Na2CO3(s) D. Na2(s) + C(s, graphite) + 1.5 O2(g) → Na2CO3(s) E. 2 Na(g) + C(g) + 1.5 O2(g) → Na2CO3(s)
Hydrogen is manufactured on an industrial scale by this sequence of reactions: CH, (g) + H,0 (g) CO (g)+3 H, (g) K1 CO (g) + H,0 (g)= CO, (g)+H, (g) K2 The net reaction is: CH4 (g) +2 H,0 (g) CO, (g)+4H, (g) K Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K, and K,. If you need to include any physical constants, be sure you use their standard symbols, which you'll find in the ALEKS Calculator. K
4. Imagine that you are given 0.2500 g of a sample of copper(II) sulfate pentahydrate (CuSO4 • 5 H2O). You very carefully heat the compound for an extended period of time to drive off water, after which you determine the mass of the remaining solid to be 0.1598 g. (i) Determine whether the data given confirm the formula of the hydrate. You must (ii) show any relevant calculations that support your answer.
The complete combustion of gasoline (C8H18) is best represented by which of the following equations: 2 C8H18 (l) + 25 O2 (g) → 16 CO2 (g) + 18 H2O(l) 2 C8H18 (l) + 17 O2 (g) → 16 CO (g) + 9 H2O (l) C8H18 (l) → 8 C (s) + 9 H2 (g) C8H18 (l) + O2(g) → 8 CO2 (g) + 9 H2O (l) C8H18 (l) + O(g) → 8 CO2 (g) + 9 H2O (l)
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.
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: 2 Cu₂ S(s) + 3 0₂(g) →2 Cu₂O(s) +2 SO₂ (g) In the second step, copper(I)oxide and carbon react to form copper and carbon monoxide: Cu₂O(s) + C(s)→2 Cu(s)+CO(g) Write the net chemical equation for the production of copper from copper(I) sulfide, oxygen and carbon. Be sure your equation is balanced. ローロ 06
[References] nelling salts," which are used to revive someone who has fainted, typically contain ammonium carbonate, (NH4)2 CO3 . Ammon. ponate decomposes readily to form ammonia, carbon dioxide, and water. The strong odor of the ammonia usually restores conscio person who has fainted. The unbalanced equation is (NH4)2 CO3(s) → NH3(9) + CO2(g) + H2O(g) alculate the mass of ammonia gas that is produced if 2.40 g of ammonium carbonate decomposes completely. g NH3 Submit Answer Try Another Version 1 item attempt remaining