Electrolysis of an aqueous solution of $$AgN{O_3}$$ with silver electrodes produces $$\underline {\left( {\text{i}} \right)} $$ at cathode while $$\underline {\left( {{\text{ii}}} \right)} $$ ions are dissolved from anode. When $$Pt$$ electrodes are used $$\underline {\left( {{\text{iii}}} \right)} $$ is produced at anode and $$\underline {\left( {{\text{iv}}} \right)} $$ at cathode.
(i)
(ii)
(iii)
(iv)
(a)
$${H_2}$$
$$NO_3^ - $$
$$O{H^ - }$$
$${H_2}$$
(b)
$$Ag$$
$${H^ + }$$
$${O_2}$$
$${H_2}$$
(c)
$$Ag$$
$$A{g^ + }$$
$${O_2}$$
$$Ag$$
(d)
$$Ag$$
$${H^ + }$$
$$A{g^ + }$$
$${O_2}$$
A.
(a)
B.
(b)
C.
(c)
D.
(d)
Answer :
(c)
Releted MCQ Question on Physical Chemistry >> Electrochemistry
Releted Question 1
The standard reduction potentials at $$298 K$$ for the following half reactions are given against each
$$\eqalign{
& Z{n^{2 + }}\left( {aq} \right) + 2e \rightleftharpoons Zn\left( s \right)\,\,\,\,\,\,\,\,\, - 0.762 \cr
& C{r^{3 + }}\left( {aq} \right) + 2e \rightleftharpoons Cr\left( s \right)\,\,\,\,\,\,\,\,\, - 0.740 \cr
& 2{H^ + }\left( {aq} \right) + 2e \rightleftharpoons {H_2}\left( g \right)\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,0.000 \cr
& F{e^{3 + }}\left( {aq} \right) + 2e \rightleftharpoons F{e^{2 + }}\left( {aq} \right)\,\,\,\,\,\,\,\,0.770 \cr} $$
which is the strongest reducing agent ?
A solution containing one mole per litre of each $$Cu{\left( {N{O_3}} \right)_2};AgN{O_3};H{g_2}{\left( {N{O_3}} \right)_2};$$ is being electrolysed by using inert electrodes. The values of standard electrode potentials in volts (reduction potentials) are :
$$\eqalign{
& Ag/A{g^ + } = + 0.80,\,\,2Hg/H{g_2}^{ + + } = + 0.79 \cr
& Cu/C{u^{ + + }} = + 0.34,\,Mg/M{g^{ + + }} = - 2.37 \cr} $$
With increasing voltage, the sequence of deposition of metals on the cathode will be :