Electrochemistr...

An electrochemical cell can behave like an electrolytic cell when:

In the electrolysis of aqueous sodium chloride solution which of the half-cell reaction will occur at the anode?

The reaction, $$2B{r^ - }\left( {aq} \right) + S{n^{2 + }}\left( {aq} \right) \to B{r_2}\left( 1 \right) + Sn\left( s \right)$$ with the standard potentials,$$E{^\circ _{Sn}} =  - 0.114V,\,E{^\circ _{B{r_2}}} =  + 1.09V$$, is:

Which of the following relation is not correct?

Chromium metal can be plated out from an acidic solution containing $$CrO_3$$ according to the following equation $$CrO_3(aq)+6H^+(aq)+6e^-\rightarrow Cr(s)+3H_2O$$
Calculate how many grams of chromium will be placed out by $$24000$$ coulombs (Atomic Weight of Cr$$=52$$).

What would you observe if you set up the following electrochemical cell
$${\text{Ag|Agn}}{{\text{o}}_3}\left( {0.001M} \right)||AgN{O_3}(1M)|Ag$$

A constant electric current flows for 4 hours through two electrolytic cells connected in series. One contains $$AgNO_3$$ solution and second contains $$CuCl_2$$ solution. During this time, 4 grams of $$Ag$$ is deposited in the first cell. How many grams of Cu is deposited in the second cell?

$$Cd$$ amalgam is prepared by electrolysis of a solution of $$CdCl_2$$ using a mercury cathode. Current of how much ampere must be passed for $$100$$ seconds in order to prepare $$20\%$$ $$Cd-Hg$$ amalgam on a cathode of $$2$$ g mercury? (At. wt. of Cd$$=112.40$$)

Given below are the half-cell reactions:
$$Mn^{2+} + 2e^- \to Mn; E^o = -1.18V$$
$$2(Mn^{3+} + e^- \to Mn^{2+}); E^o = +1.51V$$
The $$E^o$$ for $$3Mn^{2+} \to Mn +2Mn^{3+}$$ will be: