When theAg concentration is 1.50 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 1.611 V. What is theCr³+ concentration?3Ag+ (aq) + Cr(s) → 3Ag(s) + Cr³+ (aq)=→ Ag(s) E = 0.799 VredAg+ (aq) + eCr³+ (aq) + 3e¯ → Cr(s) Ee= -0.740 Vred[Cr³+] = 0M When the Ag* concentration is 2.63×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is1.324V. What is the Cr³+ concentration?3Ag*(aq) + Cr(s)- →3Ag(s) + Cr³+ (aq)Answer:M

Answered: Image /qna-images/answer/bba245e1-cf54-490e-8a4b-ca9685993498.jpg

Answered: Cr³+ concentration? 3Ag+ (aq) + Cr(s) →…

Cr³+ concentration? 3Ag+ (aq) + Cr(s) → 3Ag(s) + Cr³+ (aq) red Ag+ (aq) + e → Ag(s) = 0.799 V Cr3+ (aq) + 3e¯ → Cr(s) Fred = -0.740 V [Cr³+] = M

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

When the
Ag concentration is 1.50 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 1.611 V. What is the
Cr³+ concentration?
3Ag+ (aq) + Cr(s) → 3Ag(s) + Cr³+ (aq)
=
→ Ag(s) E = 0.799 V
red
Ag+ (aq) + e
Cr³+ (aq) + 3e¯ → Cr(s) Ee
= -0.740 V
red
[Cr³+] = 0
M

When the Ag* concentration is 2.63×10-4 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is
1.324V. What is the Cr³+ concentration?
3Ag*(aq) + Cr(s)- →3Ag(s) + Cr³+ (aq)
Answer:
M

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