electrochemistry

Related Questions

• If the half cell reaction $A+{{e}^{-}}\to {{A}^{-}}$ has a large negative reduction potential, it follows that

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• Electrochemical equivalent of $Cu$ in the reaction, $Cu^{2+}+2e^– \to Cu$ is

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• For the redox reaction $Zn\,(s)+C{{u}^{2+}}(0.1\,M)\to Z{{n}^{2+}}(1M)+Cu\,(s)$ taking place in a cell, $E_{\text{cell}}^{0}$ is 1.10 volt. ${{E}_{\text{cell}}}$ for the cell will be $\left( 2.303\frac{RT}{F}=0.0591 \right)$

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• Electrolysis involves oxidation and reduction respectively at

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• $Z{{n}^{2+}}+2{{e}^{-}}\to Zn(s);\,{{E}^{0}}=-0.76$; $F{{e}^{3+}}+{{e}^{-}}\to F{{e}^{2+}};\,{{E}^{0}}=-0.77$; $C{{r}^{3+}}+3{{e}^{-}}\to Cr;\,{{E}^{0}}=-0.79$; ${{H}^{+}}+2{{e}^{-}}\to 1/2{{H}_{2}};\,{{E}^{0}}=0.00$; Strongest reducing agent is

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