Electrochemistr...

The standard electrode potentials $$(E_{M^+/M}^{o})$$ of four metals A, B, C and D are -1.2 V, 0.6 V, 0.85 V and -0.76 V, respectively. The increasing sequence of deposition of metals on applying potential is :

Given, $$\mathrm{E}_{\mathrm{F}\mathrm{e}^{3+}/\mathrm{F}\mathrm{e}}^{o}= -0.036\mathrm{V},\ \mathrm{E}_{\mathrm{F}\mathrm{e}^{2+}/\mathrm{F}\mathrm{e}}^{o}= -0.439 \mathrm{V}$$. The value of standard electrode potential for the change, $$\mathrm{F}\mathrm{e}^{3+}(\mathrm{a}\mathrm{q})+\mathrm{e}^{-}\rightarrow \mathrm{F}\mathrm{e}^{2+}(\mathrm{a}\mathrm{q})$$ will be:

In the electrolytic cell, flow of electrons is from:

When $$0.1$$ mol $$MnO_4^{2-}$$ is oxidised the quantity of electricity required to completely $$MnO_4^{2-}$$ to $$MnO_4{^-}$$ is:

1C electricity deposits:

In a galvanic cell electron flow will be from:

An aqueous solution of the following concentration of Acetic acid is the best conductor.

In a galvanic cell, the reactions taking place in the anodic half cell and the cathodic half cell will be:

Rusting of iron is catalysed by which of the following:

$$ Cu(S) + 2Ag^{+}(aq) \rightarrow Cu^{2+}(aq)+2Ag(S) $$

In the given reaction, the reduction half cell reaction is: