When the oxidation-reduction reaction was balanced in acidic solution. If the [H2O2] = 0.352 M, partial pressure of O2 is 2.21 atm, [K2Cr207] = 0.642 M, the [Cr3*] = 0.963 M, and the pH was measured to be 8.42 then what is the cell potential at 25°C? O2(9) + Cr** (ag) → H2O2(ag) + Cr20,2 (ag) -2.51 O 2.70 -1.74 1.90 O 2.33 3.38 -3.12 O 2.92 O -3.51 -2.14 O O O O

When the oxidation-reduction reaction was balanced in acidic solution. If the [H2O2] = 0.352 M, partial pressure of O2 is 2.21 atm, [K2Cr207] = 0.642 M, the [Cr3*] = 0.963 M, and the pH was measured to be 8.42 then what is the cell potential at 25°C? O2(9) + Cr** (ag) → H2O2(ag) + Cr20,2 (ag) -2.51 O 2.70 -1.74 1.90 O 2.33 3.38 -3.12 O 2.92 O -3.51 -2.14 O O O O

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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Qq.49. Subject :- Chemistry
When the oxidation-reduction reaction was balanced in acidic solution. If the [H2O2] = 0.352 M, partial pressure of Oz is 2.21 atm, [K2Cr2O7) = 0.642 M, the [Cr3+] = 0.963 M, and the pH was measured to be 8.42 then what is the cell potential at 25°C? O2(g) + Cr3+ *(aq) → H202(aq) + Cr20-2" (aq)
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