Iron is one of our most important metals since it is cheap and very abundant. Iron canalso be mixed with other metals and carbon to produce alloys with specific properties.Many reactions occur in the blast furnace to produce iron, Fe). In the reaction thatfollows, carbon monoxide, CO(g), which is produced by oxidation of carbon, C(s), reactswith FeO (s).FeO(s) + CO() Fen + CO2(g)Which is the reducing agent in the reaction?a) Femb)CO(g)Which is the oxidizing agent in this reaction?a)Fe(1)CO(g)5.6.b)c)c)FeO(s)FeO (s)d) CO2(g)d)CO2(g)

In the given reaction:FeO + CO -> Fe + CO2The reducing agent is the species that donates…

Iron is one of our most important metals since it is cheap and very abundant. Iron can also be mixed with other metals and carbon to produce alloys with specific properties. Many reactions occur in the blast furnace to produce iron, Fea). In the reaction that follows, carbon monoxide, CO(g), which is produced by oxidation of carbon, C(s), reacts with FeO (s). FeO(s) + CO() Fen + CO2(g) Which is the reducing agent in the reaction? a) Fem b) CO(g) Which is the oxidizing agent in this reaction? a)Fe(1) b) CO(g) 5. 6. c) c) FeO(s) FeO(s) d) d) CO2(8) CO2(g)

Iron is one of our most important metals since it is cheap and very abundant. Iron can also be mixed with other metals and carbon to produce alloys with specific properties. Many reactions occur in the blast furnace to produce iron, Fea). In the reaction that follows, carbon monoxide, CO(g), which is produced by oxidation of carbon, C(s), reacts with FeO (s). FeO(s) + CO() Fen + CO2(g) Which is the reducing agent in the reaction? a) Fem b) CO(g) Which is the oxidizing agent in this reaction? a)Fe(1) b) CO(g) 5. 6. c) c) FeO(s) FeO(s) d) d) CO2(8) CO2(g)

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 to analyze for the amount of phosphorus in a rock is to precipitate the phosphorus as MgNH4PO4, which is then heated to turn it into Mg2P2O7. What weight of Mg2P2O7 will be obtained from a 2.832 g sample of a rock that contains 86.52% Ca3(PO4)2 (and no other source of phosphorus) if this analysis is done?
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There are two steps in the extraction of copper metal from chalcocite, a copper ore. In the first step, copper(1) sulfide and oxygen react to form copper(I) oxide and sulfur dioxide: 2Cu,S(s)+30,(9) --2Cu,0(3)+2SO,(9) In the second step, copper(I) oxide and carbon react to form copper and carbon monoxide: Cu,O(s)+C(s)-+2Cu(s)-co(0) Write the net chemical equation for the production of copper from copper(1) sulfide, oxygen and carbon. Be sure your equation is balanced.
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Magnesium nitrate and barium nitrate decompose similarly on heating and the reaction can be represented as follow: M(NO3)2 (s) --› MO (s) + 2NO2 (g) + ½O2 (g), where M = Mg or Ba (a) When Group 1 nitrates (with the exception of lithium nitrate) are strongly heated, the corresponding nitrite was formed along with a colorless gas which relights a glowing splint. (i) Write a balanced equation for the thermal decomposition of potassium nitrate. (ii) Unlike other Group 1 nitrates, lithium nitrate decomposes on heating in the same way as Group 2 nitrates. Suggest a reason for the difference in behaviour, and give an equation for its decomposition. (b) Zinc carbonate and magnesium carbonate decompose when heated to give similar products. (i) Suggest an equation for the thermal decomposition of magnesium carbonate. (ii) The radius of Zn2+ cation is 0.074 nm. Use the Data Booklet to deduce whether zinc carbonate will decompose at a higher or lower temperature than magnesium carbonate. Explain…
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