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4) Consider the following redox reactions and their standard cell potentials: C2(g) + BiO*(aq) = Bi(s)+ HCIO(aq) SO, (aq) + O3(g) = S,0 (aq) + 0(g) S20, (aq) + C2(g) = HCIO(aq) + SO, (aq) cell = -1.31 V E°cell = +0,10 V E°cell = +0.37 V E° (acidic conditions) (basic conditions) (acidic conditions) a) Using the ½ rxn method, balance the three redox reactions under the conditions indicated. telp b))Write each balanced redox reaction in the spontaneous direction and indicate its corresponding standard cell potential.

4) Consider the following redox reactions and their standard cell potentials: C2(g) + BiO*(aq) = Bi(s)+ HCIO(aq) SO, (aq) + O3(g) = S,0 (aq) + 0(g) S20, (aq) + C2(g) = HCIO(aq) + SO, (aq) cell = -1.31 V E°cell = +0,10 V E°cell = +0.37 V E° (acidic conditions) (basic conditions) (acidic conditions) a) Using the ½ rxn method, balance the three redox reactions under the conditions indicated. telp b))Write each balanced redox reaction in the spontaneous direction and indicate its corresponding standard cell potential.

Chemistry
Chemistry
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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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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TURE LEGAL PADS Letter Size, 8/2 x11% 50 Sheets, White PRODUCT IS RECYCLED AND RECYGLABLE 00864 VER. O35255 008648 Manufactured for S. P. Richards Co., Allanta, GA reduced 4) Consider the following redox reactions and their standard cell potentials: C2(g) + BiO*(aq) = Bi(s) + HCIO(aq) SO, (aq) + O3(g) = S20; (aq) + O2(g) S20g (aq) + Cl2(g) = HC10(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. so? (aq) telp 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.)
Transcribed Image Text:TURE LEGAL PADS Letter Size, 8/2 x11% 50 Sheets, White PRODUCT IS RECYCLED AND RECYGLABLE 00864 VER. O35255 008648 Manufactured for S. P. Richards Co., Allanta, GA reduced 4) Consider the following redox reactions and their standard cell potentials: C2(g) + BiO*(aq) = Bi(s) + HCIO(aq) SO, (aq) + O3(g) = S20; (aq) + O2(g) S20g (aq) + Cl2(g) = HC10(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. so? (aq) telp 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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