+2 t-4) Consider the following redox reactions and their standard cell potentials:(acidic conditions)(basic conditions)S,0, (aq) + Cl2(g) = HCI0(aq) + So,"(aq) (acidic conditions)cell =-1.31 VE°cell = +0.10 VE° cell = +0.37 VE°.C2(g) + Bio*(aq) = Bi(s)+ HCIO(aq)So(aq) + 03(g) = S20 (aq) + 02(g)a) Using the ½ rxn method, balance the three redox reactions under the conditions indicated.b) Write each balanced redox reaction in the spontaneous direction and indicate its correspondingstandard cell potential.c) Between these 3 redox reactions there are FOUR oxidizing agents and FOUR reducing agents.(Hint: You may need to consider the balanced equations.)i) Place the FOUR oxidizing agents in order of decreasing oxidizing strength.(From the strongest OA to the weakest OA.)ii) Place the FOUR reducing agents in order of decreasing reducing strength. ((From the strongest RA to the weakest RA.)

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4) Consider the following redox reactions and their standard cell potentials: CL(g) + BiO*(aq) Bi(s)+ HCIO(aq) So? (aq) + 0:(g) = S;0,(aq) + 0(g) S,0 (aq) + Cl2(g) = HCI0(aq) + SO?"(aq) (acidic conditions) (basic conditions) (acidic conditions) E°cell = -1.31 V E° cell +0.10 V E°cell = +0.37 V a) Using the ½ rxn method, balance the three redox reactions under the conditions indicated.

4) Consider the following redox reactions and their standard cell potentials: CL(g) + BiO*(aq) Bi(s)+ HCIO(aq) So? (aq) + 0:(g) = S;0,(aq) + 0(g) S,0 (aq) + Cl2(g) = HCI0(aq) + SO?"(aq) (acidic conditions) (basic conditions) (acidic conditions) E°cell = -1.31 V E° cell +0.10 V E°cell = +0.37 V a) Using the ½ rxn method, balance the three redox reactions under the conditions indicated.

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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Question

+2 t-
4) Consider the following redox reactions and their standard cell potentials:
(acidic conditions)
(basic conditions)
S,0, (aq) + Cl2(g) = HCI0(aq) + So,"(aq) (acidic conditions)
cell =-1.31 V
E°cell = +0.10 V
E° cell = +0.37 V
E°.
C2(g) + Bio*(aq) = Bi(s)+ HCIO(aq)
So(aq) + 03(g) = S20 (aq) + 02(g)
a) Using the ½ rxn method, balance the three redox reactions under the conditions indicated.
b) Write each balanced redox reaction in the spontaneous direction and indicate its corresponding
standard cell potential.
c) Between these 3 redox reactions there are FOUR oxidizing agents and FOUR reducing agents.
(Hint: You may need to consider the balanced equations.)
i) Place the FOUR oxidizing agents in order of decreasing oxidizing strength.
(From the strongest OA to the weakest OA.)
ii) Place the FOUR reducing agents in order of decreasing reducing strength. (
(From the strongest RA to the weakest RA.)

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