Electrolytic Cells and Electrolysis

Which of the following chemical equations are balanced:

 (i)  $2{\mathrm{MnO}}_4^{-}\left(\mathrm{aq}\right)+5{\mathrm{C}}_2{\mathrm{O}}_4^{2-}\left(\mathrm{aq}\right)+16{\mathrm{H}}^{+}\left(\mathrm{aq}\right)\to 2{\mathrm{Mn}}^{2+}\left(\mathrm{aq}\right)+8{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)+10{\mathrm{CO}}_2\left(\mathrm{g}\right)$

(ii)  ${\mathrm{Cr}}_2{\mathrm{O}}_7^{2-}\left(\mathrm{aq}\right)+6{\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right)+14\text{}{\mathrm{H}}^{+}\left(\mathrm{aq}\right)\to 2\text{}{\mathrm{Cr}}^{3+}\left(\mathrm{aq}\right)+6{\mathrm{Fe}}^{3+}\left(\mathrm{aq}\right)+7{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

On electrolysis of an aqueous solution of $\mathrm{NaCl}$, the products released at cathode and anode are, respectively

Copper sulphate solution (250 mL) was electrolysed using a platinum anode and a copper cathode. A constant current of 2 mA was passed for 16 minutes. It was found that after electrolysis the absorbance of the solution was reduced to 50% of its original value. The concentration of copper sulphate in the solution at the beginning would be:

Electrolysis of a solution of $MnS{O}_4$ in aqueous sulphuric acid is a method for the preparation of $Mn{O}_2$ as per the reaction:

${\text{Mn}}_{\text{aq}}^{2+}+2{\text{H}}_2\text{O}⟶{\text{MnO}}_{2\left(\text{s}\right)}+2{\text{H}}_{\left(\text{aq}\right)}^{+}+{\text{H}}_{2\left(\text{g}\right)}$

Passing a current of 27 A for 24 hours gives only 1 kg of $Mn{O}_2.$ The value of current efficiency would be: $\left({\text{M}}_{{\text{MnO}}_2}=86.9\text{g}\right)$

The following electrochemical cell has been set up.

$\begin{array}{l}\mathrm{Pt}\left(1\right)|{\mathrm{Fe}}^{3+},{\mathrm{Fe}}^{2+}(\mathrm{a}=1)||{\mathrm{Ce}}^{4+},{\mathrm{Ce}}^{3+}(\mathrm{a}=1\left)\right|\mathrm{Pt}\left(2\right)\\ \mathrm{E}°({\mathrm{Fe}}^{3+},{\mathrm{Fe}}^{2+})=0.77\mathrm{V}:\mathrm{E}°({\mathrm{Ce}}^{4+},{\mathrm{Ce}}^{3+})=1.61\mathrm{V}\end{array}$
If an ammeter is connected between the two platinum electrodes, predict the direction of flow of current.

In the electrolytic cell, flow of electrons is from:

Electric current was passed through an aqueous solution of ${\mathrm{CuSO}}_4$ using two $\mathrm{Pt}$ electrodes. After some time, the blue colour of the solution disappeared along with evolution of ${\mathrm{O}}_2$ gas. Which of the following statement is correct regarding the resultant solution?

Electrolysis is used for

In electrochemical cell, oxidation and reduction occurs at

Which of the following statements is not applicable to electrolytic conductors?

Faraday's of electricity required to reduce 1 mole of ${\mathrm{MnO}}_4^{-}$ ions to ${\mathrm{Mn}}^{2+}$:

In the electrolysis of molten ${\mathrm{Al}}_2{\mathrm{O}}_3$ with inert electrodes

The gas evolved at the anode when ${\mathrm{K}}_2{\mathrm{SO}}_4 \left(\mathrm{aq}\right)$ is electrolyzed between $\mathrm{Pt}$ electrodes is:

The aqueous solutions of following substances were electrolyzed. In which case the $\mathrm{pH}$ of solution doesn't change if inert electrodes are used

If an aqueous $\mathrm{NaCl}$ solution is electrolyzed which phenomenon is not observed ?

Which of the following aqueous solutions remain neutral after electrolysis?

For daniel cell reaction ${\mathrm{K}}_{\mathrm{c}}={10}^{12}$ then ${\mathrm{E}}_{\text{cell }}°$ and the cell reaction will be:-