electrochemistry

Question: Calculate the equilibrium constant of the reaction, $C{{d}^{2+}}(aq)+Zn\,(s)\to Z{{n}^{2+}}(aq)+Cd\,(s)$ If $E_{C{{d}^{2+}}/Cd}^{0}=-0.403\,V$ and $E_{Z{{n}^{2+}}/Zn}^{0}=-0.763\,V$

1) $K=1.45\times {{10}^{12}}$

2) $K=4.25\times {{10}^{14}}$

3) $K=1.45\times {{10}^{12}}$

4) $K=14.4\times {{10}^{11}}$

Solution:

Explanation: No Explanation

Electrode potential Ecell Nernst equation and ECS

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