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3) In each redox reaction indicated in equations 1-6, indicate which species is oxidized and which species is reduced..

3) In each redox reaction indicated in equations 1-6, indicate which species is oxidized and which species is reduced..

Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter18: Oxidation–reduction Reactions And Electrochemistry
Section: Chapter Questions
Problem 84AP: . For each of the following unbalanced oxidation-reduction chemical equations, balance the equation...
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1) Why is hydrochloric acid not used directly in a reaction with copper metal to produce CuCl₂? 2) What is the maximum amount of CuCl which can be produced by the procedure in this experiment if one starts with 1 g of copper metal? 3) In each redox reaction indicated in equations 1-6, indicate which species is oxidized and which species is reduced..
Transcribed Image Text:1) Why is hydrochloric acid not used directly in a reaction with copper metal to produce CuCl₂? 2) What is the maximum amount of CuCl which can be produced by the procedure in this experiment if one starts with 1 g of copper metal? 3) In each redox reaction indicated in equations 1-6, indicate which species is oxidized and which species is reduced..
(Eq. 1) (Eq. 2) (Eq. 3) (Eq. 4) (Eq. 5) (Eq. 6) Cus) + 4 H* (aq) + 2NO3(aq) → Cu²+ (aq) + 2 NO₂(g) + 2 H₂O 2 H* (aq) + CO3² (aq) = H₂CO3(aq) CO2(g) + H₂O Cu²+ (aq) + CO3(aq) CuCO3(6) CUCO3(s) + 2 H+ (aq) + 4 Cl(aq) →CuCl(aq) + CO2(g) + H₂O CuCl(aq) + Cu(s) + 4 Cl(aq)-2 CuCl4³(aq) CuCl(aq) → CuClo) + 3 Cl(aq)
Transcribed Image Text:(Eq. 1) (Eq. 2) (Eq. 3) (Eq. 4) (Eq. 5) (Eq. 6) Cus) + 4 H* (aq) + 2NO3(aq) → Cu²+ (aq) + 2 NO₂(g) + 2 H₂O 2 H* (aq) + CO3² (aq) = H₂CO3(aq) CO2(g) + H₂O Cu²+ (aq) + CO3(aq) CuCO3(6) CUCO3(s) + 2 H+ (aq) + 4 Cl(aq) →CuCl(aq) + CO2(g) + H₂O CuCl(aq) + Cu(s) + 4 Cl(aq)-2 CuCl4³(aq) CuCl(aq) → CuClo) + 3 Cl(aq)
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