An iron wire is immersed in a solution containing ZnSO₄ and NiSO₄. The concentration of each salt is 1 M. Predict, giving reasons, which of the following reactions is likely to proceed:(i) Iron reduces Zn²⁺ ions (ii) Iron reduces Ni²⁺ ionsGiven: \( E^\circ_{(Zn^{2+}/Zn)} = -0.76 \, \text{V} \) \( E^\circ_{(Fe^{2+}/Fe)} = -0.44 \, \text{V} \) \( E^\circ_{(Ni^{2+}/Ni)} = -0.25 \, \text{V} \)

Given that, an iron wire is immersed in a solution containing ZnSO4 and NiSO4. Also, the…

An iron wire is immersed in a solution containing ZnSO, and NiSO. The concentration of each salt is 1 M. Predict, giving reasons, which of the following reaction is likely to proceed. (i) Iron reduces Zn²+ ions (ii) Iron reduces Ni²+ ions, Given: E²Z) = -0.76V; (Zn) EFF) = -0.44 V; ENN)=-0.25 V (Fe /Fe)

An iron wire is immersed in a solution containing ZnSO, and NiSO. The concentration of each salt is 1 M. Predict, giving reasons, which of the following reaction is likely to proceed. (i) Iron reduces Zn²+ ions (ii) Iron reduces Ni²+ ions, Given: E²Z) = -0.76V; (Zn) EFF) = -0.44 V; ENN)=-0.25 V (Fe /Fe)

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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Show solution also on the part of answering whether the reaction is spontaneous or not.
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