Consider a galvanic electrochemical cell constructed using Cr/Cr**and Zn/Zn2* at 25 °C. The following half-reactions are provided foreach metal:Cre(aq) + 3 е >Zn²*(aq) + 2 e → Zn(s) E°red = -0.763 VCr(s) E°red = -0.744 VWhich of the following is the half-reaction that takes place at theanode.A) Cr*(aq) + 3 e → Cr(s)B) Cr(s) –Cr*(aq) + 3 eC) Zn²(aq) + 2 e→ Zn(s)D) Zn(s) → Zn²*(aq) + 2 e

The anode is present on the left side of the electrochemical cell and at the anode, oxidation is takes place The electrode whose Oxidation potential is major is place at anode. The electrode whose reduction potential is less is place at anode. Out of Cr+3 and Zn+2 the reduction potential of Zn+2 is minimum due to this Zn+2 is acted as anode. Also the Oxidation potential is maximum for Zn than the Cr Hence option D is right answer Zn(s) -------------> Zn(aq)+2 + 2e-

Science

Chemistry

Consider a galvanic electrochemical cell constructed using Cr/Cr** and Zn/Zn2* at 25 °C. The following half-reactions are provided for each metal: Cr**(aq) + 3 e → Cr(s) E°red = -0.744 V Zn2*(aq) + 2 e → Zn(s) E°red = -0.763 V %3D Which of the following is the half-reaction that takes place at the anode. А) Cr(aq) + 3е — Cr(s) B) Cr(s) → Cr*(aq) + 3 e C) Zn² (aq) + 2 e → Zn(s) D) Zn(s) → Zn2(aq) + 2 e

Consider a galvanic electrochemical cell constructed using Cr/Cr** and Zn/Zn2* at 25 °C. The following half-reactions are provided for each metal: Cr**(aq) + 3 e → Cr(s) E°red = -0.744 V Zn2(aq) + 2 e → Zn(s) E°red = -0.763 V %3D Which of the following is the half-reaction that takes place at the anode. А) Cr(aq) + 3е — Cr(s) B) Cr(s) → Cr(aq) + 3 e C) Zn² (aq) + 2 e → Zn(s) D) Zn(s) → Zn2(aq) + 2 e

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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