plea,se helpp An electrochemical cell is based on these two half-reactions and their given standard reduction potential values:Ox: Sn (s)Red: C1O2 (g, 0.270 bar) + e¯ → Cio, (aq, 1.80 mol L-1) Eathode = 0.95 (V)→ Sn²+ (aq, 1.50 mol L-1) +2 e-E°= -0.14 (V)'anode%3DPart ACompute the cell potential at 25 °C.Express your answer to two decimal places and include the appropriate units.µA圈]?Ecell = 1.01VSubmitPrevious Answers Request AnswerX Incorrect; Try Again; One attempt remainingReview your calculations and make sure you round to 3 significant figures in the last step.

Answered: Image /qna-images/answer/ac752d16-a816-45a9-be43-282095143c55.jpg

An electrochemical cell is based on these two half-reactions and their given standard reduction potential values: Ox: Sn (s) Sn²+ (aq, 1.50 mol L-1) +2 e¯ E° anode = -0.14 (V) Red: CIO2 (g, 0.270 bar) +e¯ → ClO, (aq, 1.80 mol L-!) Eº cathode = 0.95 (V)

An electrochemical cell is based on these two half-reactions and their given standard reduction potential values: Ox: Sn (s) Sn²+ (aq, 1.50 mol L-1) +2 e¯ E° anode = -0.14 (V) Red: CIO2 (g, 0.270 bar) +e¯ → ClO, (aq, 1.80 mol L-!) Eº cathode = 0.95 (V)

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

plea,se helpp

An electrochemical cell is based on these two half-reactions and their given standard reduction potential values:
Ox: Sn (s)
Red: C1O2 (g, 0.270 bar) + e¯ → Cio, (aq, 1.80 mol L-1) Eathode = 0.95 (V)
→ Sn²+ (aq, 1.50 mol L-1) +2 e-
E°
= -0.14 (V)
'anode
%3D
Part A
Compute the cell potential at 25 °C.
Express your answer to two decimal places and include the appropriate units.
µA
圈]
?
Ecell = 1.01
V
Submit
Previous Answers Request Answer
X Incorrect; Try Again; One attempt remaining
Review your calculations and make sure you round to 3 significant figures in the last step.

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