Question

The given figure shows the corrosion of iron in atmosphere,
Electrochemistry mcq question image
Fill in the blanks by choosing an appropriate option. At a particular spot of an object made of iron, $$\underline {\left( {\text{i}} \right)} $$  of iron to ferrous ion takes place and that spot behaves as $$\underline {\left( {{\text{ii}}} \right)} $$  . Electrons released at anodic spot move through the metal and go to another spot on the metal and reduce oxygen in presence of $${H^ + }.$$  This spot behaves as $$\underline {\left( {{\text{iii}}} \right)} \,$$  . The ferrous ions are further oxidised by atmospheric oxygen to ferric ions which come out as rust, $$\underline {\left( {{\text{iv}}} \right)} $$  and with further production of $$\underline {\left( {\text{v}} \right)} $$  ions.
(i) (ii) (iii) (iv) (v)
(a) oxidation anode cathode Fe2O3.xH2O hydrogen
(b) reduction cathode anode Fe3O4 hydroxide
(c) oxidation cathode anode Fe2O3.xH2O hydrogen
(d) oxidation anode cathode Fe2O3.H2O ferrous

A. (a)  
B. (b)
C. (c)
D. (d)
Answer :   (a)

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. $$Zn\left( s \right)$$
B. $$Cr\left( s \right)$$
C. $${H_2}\left( g \right)$$
D. $$F{e^{2 + }}\left( {aq} \right)$$
View Answer
Releted Question 2

Faraday’s laws of electrolysis are related to the

A. atomic number of the reactants.
B. atomic number of the anion.
C. equivalent weight of the electrolyte.
D. speed of the cation.
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Releted Question 3

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 :

A. $$Ag,Hg,Cu,Mg$$
B. $$Mg,Cu,Hg,Ag$$
C. $$Ag,Hg,Cu$$
D. $$Cu,Hg,Ag$$
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Releted Question 4

The electric charge for electrode deposition of one gram equivalent of a substance is :

A. one ampere per second.
B. 96,500 coloumbs per second.
C. one ampere for one hour.
D. charge on one mole of electrons.
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