Which statement is true for the following reaction:Fe203 + C - Fe + CO2O Fe,03 is the reducing agent, since it is reduced, while C is the oxidizing agent,since it oxidizes Fe203.O Fe203 is the reducing agent, while Fe is the oxidizing agent, as it oxidizes C toCO2.O Fe is the reducing agent, since it reduces C, while C is the oxidizing agent.O Fe,03 is the oxidizing agent, while C is the reducing agent, since it reducesFe2O3.O Fe203 is the reducing agent, while CO, is the oxidizing agent.

Answered: Image /qna-images/answer/bb984e2c-224d-4dc8-a227-4f2f27ec5514.jpg

Which statement is true for the following reaction: Fe203 + C - Fe + CO2 O Fe203 is the reducing agent, since it is reduced, while C is the oxidizing agent, since it oxidizes Fe203. O Fe203 is the reducing agent, while Fe is the oxidizing agent, as it oxidizes C to CO2. Fe is the reducing agent, since it reduces C, while C is the oxidizing agent. O Fe203 is the oxidizing agent, while C is the reducing agent, since it reduces Fe203. O Fe203 is the reducing agent, while CO, is the oxidizing agent.

Which statement is true for the following reaction: Fe203 + C - Fe + CO2 O Fe203 is the reducing agent, since it is reduced, while C is the oxidizing agent, since it oxidizes Fe203. O Fe203 is the reducing agent, while Fe is the oxidizing agent, as it oxidizes C to CO2. Fe is the reducing agent, since it reduces C, while C is the oxidizing agent. O Fe203 is the oxidizing agent, while C is the reducing agent, since it reduces Fe203. O Fe203 is the reducing agent, while CO, is the oxidizing agent.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 22P

See similar textbooks

Similar questions

Balance the following oxidationreduction equations. The reactions occur in acidic or basic aqueous solution, as indicated. a MnO4+IMnO2+IO3(basic) b Cr2O32+ClCr3++Cl2(acidic) c S8+NO3SO2+NO(acidic) d H2O2+MnO4O2+MnO2(basic) e Zn+NO3Zn2++N2(acidic)
Copper(I) ion disproportionates to copper metal and copper(ll) ion. (See Study Question 99.) 2 Cu+(aq) Cu(s) + Cu2 + (aq) (a) What two half-reactions make up the disproportionation reaction? (b) Use values of the standard reduction potentials for the two half-reactions in part (a) to determine whether this disproportionation reaction is product-favored at equilibrium. (c) What is the equilibrium constant for this reaction? If you have a solution that initially contains 0.10 mol of Cu+ in 1.0 L of water, what are the concentrations of Cu+ and Cu2+ at equilibrium?
The Ostwald process for the commercial production of nitric acid involves the Following three steps: 4NH3(g)+5O2(g)4NO(g)+6H2O(s)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(aq)+NO(g) a. Which reaction in the Ostwald process are oxidation-reduction reactions? b. Identify each oxidizing agent and reducing agent.
Bromine is obtained from brine wells. The process involves treating water containing bromide ion with Cl2 and extracting the Br2 from the solution using an organic solvent. Write a balanced equation for the reaction of Cl2 and Br. What are the oxidizing and reducing agents in this reaction? Using the table of standard reduction potentials (Appendix M), verify that this is a product-favored reaction at equilibrium.
(a) Write equations for the half-reactions that occur at the cathode and the anode when an aqueous solution of KCl is electrolyzed. Which chemical species is oxidized, and which chemical species is reduced in this reaction? (b) Predict the products formed when an aqueous solution of CsI is electrolyzed.
The halogen oxides and oxoanions are good oxidizing agents. For example, the reduction of bromate ion has an E value of 1.44 V in acid solution: 2BrO3(aq)+12H+(aq)+10eBr2(aq)+6H2O(l) Is it possible to oxidize aqueous 1.0 M Mn2+ to aqueous MnO4 with 1.0 M bromate ion?
Iron(II) can be oxidized to iron(III) by permanganate ion in acidic solution. The permanganate ion is reduced to manganese(II) ion. (a) Write the oxidation half-reaction, the reduction half-reaction, and the overall redox equation. (b) Calculate E° for the reaction. (c) Calculate the percentage of Fe in an ore if a 0.3500-g sample is dissolved and the Fe2+ formed requires for titration 55.63 mL of a 0.0200 M solution of KMnO4.
Iron(II) ion undergoes a disproportionation reaction to give Fe(s) and the iron(III) ion. That is, iron(II) ion is both oxidized and reduced within the same reaction. 3 Fe2+(aq) Fe(s) + 2 Fe3+(aq) (a) What two half-reactions make up the disproportionation reaction? (b) Use the values of the standard reduction potentials for the two half-reactions in part (a) to determine whether this disproportionation reaction is product-favored at equilibrium. (c) What is the equilibrium constant for this reaction?