Electrochemistr...

The figure shows a car bumper coated with chromium.

Why are car bumpers often coated with chromium?

 1 faraday is defined as:

Which cell involves spontaneous oxidation and reduction?

The given diagram shows an electrochemical cell in which the respective half cells contain aqueous 1.0 M solutions of the salts $$XCl_2$$ and $$YCl_3$$. Given that, 

The concentration of potassium ions inside a biological cell is at least twenty times higher than the outside. The resulting potential difference across the cell is important in several processes such as transmission of nerve impulses and maintaining the ion balance. A simple model for such a concentration cell involving a metal M is:
$$\mathrm{M}(\mathrm{s})|\mathrm{M}^{+}(\mathrm{a}\mathrm{q};0.05\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{a}\mathrm{r})||\mathrm{M}^{+}(\mathrm{a}\mathrm{q})$$ , 1 $$\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{a}\mathrm{r})|\mathrm{M}(\mathrm{s})$$
For the above electrolytic cell the magnitude of the cell potential $$|\mathrm{E}_{\mathrm{c}\mathrm{e}ll}|=70\mathrm{m}\mathrm{V}$$.

What is $$E_{RP}^0$$ for the reaction : $$C{u^{2 + }} + 2e\xrightarrow{{}}Cu$$ in the half cell $$P{t_{{S^{2 - }}/CuS/Cu}}$$ if $$E_{C{u^{2 + }}/Cu}^0$$ is 0.34 V and $$K_{sp}$$ of $$CuS=10^{-35}$$ ?

In a voltaic cell, if iron and silver electrodes are connected with each other then current flows:

The electrode potentials for $$Cu^{2+}_{(aq)} + e^{-} \rightarrow Cu_{(aq)}^{+}$$ and $$Cu_{(aq)}^{+} + e^{-} \rightarrow Cu_{(s)}$$
Are $$+0.15 V$$ and $$+0.50 V$$ respectively.
The value of $$E_{Cu^{2+}/Cu}^{\circ}$$ will be

In a daniel cell, if $$A(E^o = -0.76 \ C)$$ and $$B(E^o = -2.36 \ V)$$ half cells are taken then:

At 300K, $$\Delta$$H for the reaction $$Zn(s) + 2AgCl \rightarrow ZnCl_2 + 2Ag$$, is $$- 218$$ kJ/mol while the emf of the cell was $$1.015V$$. $$(\dfrac{dE}{dT})_p$$ of the cell is :