electrochemistry

Related Questions

• A solution containing one mole per litre of each $Cu{{(N{{O}_{3}})}_{2}},\,AgN{{O}_{3}},\,H{{g}_{2}}{{(N{{O}_{3}})}_{2}}$ and $Mg{{(N{{O}_{3}})}_{2}}$, is being electrolysed by using inert electrodes. The values of standard electrode potentials in volts (reduction potentials) are $Ag/A{{g}^{+}}=+0.80,$ $2Hg/Hg_{2}^{2+}=+0.79,$ $Cu/C{{u}^{2+}}=+0.34,\,Mg/M{{g}^{2+}}=-2.37$ with increasing voltage, the sequence of deposition of metals on the cathode will be

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• Electrolysis rules of Faraday's states that mass deposited on electrode is proportional to

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• The chemical reaction taking place at the anode of a cell 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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• A standard hydrogen electrode has zero electrode potential because

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