Calculate \( K_c \) for the system \( \text{Ni}^{2+} + \text{Co} \rightleftharpoons \text{Ni} + \text{Co}^{2+} \). Assume \( T = 298 \, \text{K} \).\[\begin{array}{|c|l|}\hlineE^\circ \, (\text{Volts}) & \text{Half-Cell Reaction} \\\hline-0.25 & \text{Ni}^{2+} (aq) + 2e^- \rightarrow \text{Ni} (s) \\-0.28 & \text{Co}^{2+} (aq) + 2e^- \rightarrow \text{Co} (s) \\\hline\end{array}\]The table lists the standard reduction potentials (\( E^\circ \)) and the corresponding half-cell reactions for nickel and cobalt.

first we will calculate the Electrode potential of the cell here we can see Ni+2 is reduced to Ni…

Answered: Calculate K. for the system Ni2+ + Co S…

Calculate K. for the system Ni2+ + Co S Ni + Co2+. Assume T = 298 K. E° (Volts) Half-Cell Reaction Ni (ag) +2e Co2" (aq) + 2e -0.25 Ni(s) -0.28 Co(s)

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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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Calculate \( K_c \) for the system \( \text{Ni}^{2+} + \text{Co} \rightleftharpoons \text{Ni} + \text{Co}^{2+} \). Assume \( T = 298 \, \text{K} \).

\[
\begin{array}{|c|l|}
\hline
E^\circ \, (\text{Volts}) & \text{Half-Cell Reaction} \\
\hline
-0.25 & \text{Ni}^{2+} (aq) + 2e^- \rightarrow \text{Ni} (s) \\
-0.28 & \text{Co}^{2+} (aq) + 2e^- \rightarrow \text{Co} (s) \\
\hline
\end{array}
\]

The table lists the standard reduction potentials (\( E^\circ \)) and the corresponding half-cell reactions for nickel and cobalt.

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