Electrochemistry PYQs - Last 10 Years
JEE Main / Chemistry / Physical Chemistry / 184 recent questions
ChemistryPhysical Chemistry2017-2026
Practice 184 JEE Main Chemistry questions from Electrochemistry. Use the year-wise and type-wise breakdown to prioritize recent PYQs, then continue into the question list below.
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Last 10 Years Electrochemistry Questions
Showing 34 of 184 filtered questions.
1Electrochemistry
The equation that is incorrect is :
MCQ+4 / -12020
2Electrochemistry
Potassium chlorate is prepared by the
electrolysis of KCl in basic solution
6OH- + Cl- \(\to\) ClO3- + 3H2O + 6e-
If only 60% of the current is utilized in the
reaction, the time (rounded to the nearest hour)
required to produce 10 g of K...
electrolysis of KCl in basic solution
6OH- + Cl- \(\to\) ClO3- + 3H2O + 6e-
If only 60% of the current is utilized in the
reaction, the time (rounded to the nearest hour)
required to produce 10 g of K...
INTEGER+4 / -02020
3Electrochemistry
For the given cell :
Cu(s) | Cu2+(C1M) || Cu2+(C2M) | Cu(s)
change in Gibbs energy (\(\Delta\)G) is negative, if :
Cu(s) | Cu2+(C1M) || Cu2+(C2M) | Cu(s)
change in Gibbs energy (\(\Delta\)G) is negative, if :
MCQ+4 / -12020
4Electrochemistry
An oxidation-reduction reaction in which 3 electrons are transferred has a \(\Delta\)Gº of 17.37 kJ mol–1 at
25 oC. The value of Eo
cell (in V) is ______ × 10–2.
(1 F = 96,500 C mol–1)
25 oC. The value of Eo
cell (in V) is ______ × 10–2.
(1 F = 96,500 C mol–1)
INTEGER+4 / -02020
5Electrochemistry
The variation of molar conductivity with concentration of an electrolyte (X) in aqueous solution
is shown in the given figure.
The electrolyte X is :
is shown in the given figure.
The electrolyte X is :
MCQ+4 / -12020
6Electrochemistry
\(E_{C{u^{2 + }}|Cu}^0\) = +0.34 V
\(E_{Z{n^{2 + }}|Zn}^0\) = -0.76 V
Identify the incorrect statement from the option
below for the above cell :
MCQ+4 / -12020
7Electrochemistry
250 mL of a waste solution obtained from the
workshop of a goldsmith contains 0.1 M AgNO3
and 0.1 M AuCl. The solution was electrolyzed
at 2V by passing a current of 1A for 15
minutes. The metal/metals electrodeposited will
be
[ $$E_{A{g^ +...
workshop of a goldsmith contains 0.1 M AgNO3
and 0.1 M AuCl. The solution was electrolyzed
at 2V by passing a current of 1A for 15
minutes. The metal/metals electrodeposited will
be
[ $$E_{A{g^ +...
MCQ+4 / -12020
8Electrochemistry
The photoelectric current from Na (Work function, w0
= 2.3 eV) is stopped by the output voltage of
the cell Pt(s) | H2
(g, 1 Bar) | HCl (aq., pH =1) | AgCl(s) | Ag(s).
The pH of aq. HCl required to stop the photoelectric current form K(w0
...
= 2.3 eV) is stopped by the output voltage of
the cell Pt(s) | H2
(g, 1 Bar) | HCl (aq., pH =1) | AgCl(s) | Ag(s).
The pH of aq. HCl required to stop the photoelectric current form K(w0
...
INTEGER+4 / -02020
9Electrochemistry
Let CNaCl
and CBaSO4 be the conductances (in S) measured for saturated aqueous solutions of NaCl
and BaSO4, respectively, at a temperature T.
Which of the following is false?
and CBaSO4 be the conductances (in S) measured for saturated aqueous solutions of NaCl
and BaSO4, respectively, at a temperature T.
Which of the following is false?
MCQ+4 / -12020
10Electrochemistry
An acidic solution of dichromate is electrolyzed
for 8 minutes using 2A current. As per the
following equation
Cr2O72-
+ 14H+ + 6e– \(\to\) 2Cr3+ + 7H2O
The amount of Cr3+ obtained was 0.104 g. The
efficiency of the process(in%) is
(Take...
for 8 minutes using 2A current. As per the
following equation
Cr2O72-
+ 14H+ + 6e– \(\to\) 2Cr3+ + 7H2O
The amount of Cr3+ obtained was 0.104 g. The
efficiency of the process(in%) is
(Take...
INTEGER+4 / -02020
11Electrochemistry
The Gibbs change (in J) for the given reaction at
[Cu2+] = [Sn2+] = 1 M and 298K is :
Cu(s) + Sn2+(aq.) \(\to\) Cu2+(aq.) + Sn(s);
(\(E_{S{n^{2 + }}|Sn}^0 = - 0.16\,V\),
\(E_{C{u^{2 + }}|Cu}^0 = 0.34\,V\))
Take F = 96500 C mol–1)
[Cu2+] = [Sn2+] = 1 M and 298K is :
Cu(s) + Sn2+(aq.) \(\to\) Cu2+(aq.) + Sn(s);
(\(E_{S{n^{2 + }}|Sn}^0 = - 0.16\,V\),
\(E_{C{u^{2 + }}|Cu}^0 = 0.34\,V\))
Take F = 96500 C mol–1)
INTEGER+4 / -02020
12Electrochemistry
For the disproportionation reaction
2Cu+(aq) ⇌ Cu(s) + Cu2+(aq) at 298 K. ln K
(where K is the equilibrium constant) is
___________ × 10–1.
Given :
(\(E_{C{u^{2 + }}/C{u^ + }}^0 = 0.16V\)
\(E_{C{u^ + }/Cu}^0 = 0.52V\)
$${{RT} \over F} = 0.0...
2Cu+(aq) ⇌ Cu(s) + Cu2+(aq) at 298 K. ln K
(where K is the equilibrium constant) is
___________ × 10–1.
Given :
(\(E_{C{u^{2 + }}/C{u^ + }}^0 = 0.16V\)
\(E_{C{u^ + }/Cu}^0 = 0.52V\)
$${{RT} \over F} = 0.0...
INTEGER+4 / -02020
13Electrochemistry
The anodic half-cell of lead-acid battery is recharged using electricity of 0.05 Faraday. The amount of PbSO4 electrolyzed in g during the process is : (Molar mass of PbSO4 = 303 g mol\(-\)1)
MCQ+4 / -12019
14Electrochemistry
If the standard electrode potential for a cell is 2 V at 300 K, the equilibrium constant (K) for the reaction
Zn(s) + Cu2+ (aq) \(\rightleftharpoons\) Zn2+(aq) + Cu(s)
at 300 K is approximately,
(R = 8 JK\(-\)1mol\(-\)1, F = 96000 C mol$...
Zn(s) + Cu2+ (aq) \(\rightleftharpoons\) Zn2+(aq) + Cu(s)
at 300 K is approximately,
(R = 8 JK\(-\)1mol\(-\)1, F = 96000 C mol$...
MCQ+4 / -12019
15Electrochemistry
The standard Gibbs energy for the given cell
reaction in kJ mol–1 at 298 K is :
Zn(s) + Cu2+ (aq) \(\to\) Zn2+ (aq) + Cu (s),
E° = 2 V at 298 K
(Faraday's constant, F = 96000 C mol–1)
reaction in kJ mol–1 at 298 K is :
Zn(s) + Cu2+ (aq) \(\to\) Zn2+ (aq) + Cu (s),
E° = 2 V at 298 K
(Faraday's constant, F = 96000 C mol–1)
MCQ+4 / -12019
16Electrochemistry
A solution of Ni(NO3)2 is electrolysed between
platinum electrodes using 0.1 Faraday
electricity. How many mole of Ni will be
deposited at the cathode?
platinum electrodes using 0.1 Faraday
electricity. How many mole of Ni will be
deposited at the cathode?
MCQ+4 / -12019
17Electrochemistry
Given that \({E^\Theta }_{{O_2}/{H_2}O} = 1.23\,V\) ;
\({E^\Theta }_{{S_2}O_8^{2 - }/SO_4^{2 - }} = 2.05\,V\)
\({E^\Theta }_{B{r_2}/B{r^ - }} = 1.09\,V\)
\({E^\Theta }_{A{u^{3 + }}/Au} = 1.4\,V\)
The strongest oxidizing agent is :
\({E^\Theta }_{{S_2}O_8^{2 - }/SO_4^{2 - }} = 2.05\,V\)
\({E^\Theta }_{B{r_2}/B{r^ - }} = 1.09\,V\)
\({E^\Theta }_{A{u^{3 + }}/Au} = 1.4\,V\)
The strongest oxidizing agent is :
MCQ+4 / -12019
18Electrochemistry
Calculate the standard cell potential in (V) of the
cell in which following reaction takes place :
Fe2+(aq) + Ag+(aq) \(\to\) Fe3+(aq) + Ag (s)
Given that
\(E_{A{g^ + }/Ag}^o = xV\)
\(E_{Fe^{2+ }/Fe}^o = yV\)
\(E_{Fe^{3+ }/Fe}^o = zV\)
cell in which following reaction takes place :
Fe2+(aq) + Ag+(aq) \(\to\) Fe3+(aq) + Ag (s)
Given that
\(E_{A{g^ + }/Ag}^o = xV\)
\(E_{Fe^{2+ }/Fe}^o = yV\)
\(E_{Fe^{3+ }/Fe}^o = zV\)
MCQ+4 / -12019
19Electrochemistry
The standard electrode potential \({E^o }\) and its temperature coefficient \(\left( {{{d{E^o }} \over {dT}}} \right)\) for a cell are 2V and \(-\) 5 \(\times\) 10\(-\)4 VK\(-\)1 at 300 K respectively.
The cell reaction is
Zn(s) + Cu2+ ...
The cell reaction is
Zn(s) + Cu2+ ...
MCQ+4 / -12019
20Electrochemistry
\(\wedge _m^ \circ\) for NaCl, HCl and NaA are 126.4, 425.9 and 100.5 S cm2 mol–1, respectively. If the conductivity of 0.001 M HA is-
5 \(\times\) 10–5 S cm–1, degree of dissociation of HA is -
5 \(\times\) 10–5 S cm–1, degree of dissociation of HA is -
MCQ+4 / -12019
21Electrochemistry
Given
CO3+ + e– \(\to\) CO2+ ; Eo = + 1.81 V
Pb4+
+ 2e– \(\to\) Pb2+ ; Eo = + 1.67 V
Ce4+
+ e– \(\to\) Ce3+
; Eo = + 1.61 V
Bi3+ + 3e– \(\to\) Bi ; Eo = + 0.20 V
Oxidizing power of the species will increase in the order :
CO3+ + e– \(\to\) CO2+ ; Eo = + 1.81 V
Pb4+
+ 2e– \(\to\) Pb2+ ; Eo = + 1.67 V
Ce4+
+ e– \(\to\) Ce3+
; Eo = + 1.61 V
Bi3+ + 3e– \(\to\) Bi ; Eo = + 0.20 V
Oxidizing power of the species will increase in the order :
MCQ+4 / -12019
22Electrochemistry
For the cell Zn(s) |Zn2+ (aq)| |Mx+ (aq)| M(s), different half cells and their standard electrode potentials are given below :
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MCQ+4 / -12019
23Electrochemistry
Given the equilibrium constant:
KC of the reaction :
Cu(s) + 2Ag+ (aq) \(\to\) Cu2+ (aq) + 2Ag(s) is 10 \(\times\) 1015, calculate the E\(_{cell}^0\) of this reaciton at 298 K [2.303 \({{RT} \over F}\) at 298 K = 0.059V]
KC of the reaction :
Cu(s) + 2Ag+ (aq) \(\to\) Cu2+ (aq) + 2Ag(s) is 10 \(\times\) 1015, calculate the E\(_{cell}^0\) of this reaciton at 298 K [2.303 \({{RT} \over F}\) at 298 K = 0.059V]
MCQ+4 / -12019
24Electrochemistry
Consider the following reduction processes :
Zn2+ + 2e– \(\to\) Zn(s) ; Eo = – 0.76 V
Ca2+ + 2e– \(\to\) Ca(s); Eo = –2.87 V
Mg2+ + 2e– \(\to\) Mg(s) ; Eo = – 2.36 V
Ni2 + 2e– \(\to\) Ni(s) ; Eo = – 0.25
The reducing power of the m...
Zn2+ + 2e– \(\to\) Zn(s) ; Eo = – 0.76 V
Ca2+ + 2e– \(\to\) Ca(s); Eo = –2.87 V
Mg2+ + 2e– \(\to\) Mg(s) ; Eo = – 2.36 V
Ni2 + 2e– \(\to\) Ni(s) ; Eo = – 0.25
The reducing power of the m...
MCQ+4 / -12019
25Electrochemistry
In the cell
Pt\(\left| {\left( s \right)} \right|\)H2(g, 1 bar)\(\left| {HCl\left( {aq} \right)} \right|\)AgCl\(\left| {\left( s \right)} \right|\)Ag(s)|Pt(s)
the cell potential is 0.92 V when a 10–6 molal HCl solution is used. The stand...
Pt\(\left| {\left( s \right)} \right|\)H2(g, 1 bar)\(\left| {HCl\left( {aq} \right)} \right|\)AgCl\(\left| {\left( s \right)} \right|\)Ag(s)|Pt(s)
the cell potential is 0.92 V when a 10–6 molal HCl solution is used. The stand...
MCQ+4 / -12019
26Electrochemistry
Consider the statements S1 and S2
S1 : Conductivity always increases with decrease in the concentration of electrolyte.
S2 : Molar conductivity always increases with decrease in the concentration of electrolyte.
The correct option among the...
S1 : Conductivity always increases with decrease in the concentration of electrolyte.
S2 : Molar conductivity always increases with decrease in the concentration of electrolyte.
The correct option among the...
MCQ+4 / -12019
27Electrochemistry
Which one of the following graphs between molar conductivity (\({\Lambda _m}\)) versus \(\sqrt C\) is correct ?
MCQ+4 / -12019
28Electrochemistry
When 9.65 ampere current was passed for 1.0 hour into nitrobenzene in acidic medium, the amount of p-aminophenol produced is :
MCQ+4 / -12018
29Electrochemistry
When an electric currents passed through acidified water, 112 mL of hydrogen gas at N.T.P. was collected at the cathode in 965 seconds. The current passed, in ampere, is :
MCQ+4 / -12018
30Electrochemistry
How long (approximate) should water be electrolysed by passing through 100 amperes current so that the
oxygen released can completely burn 27.66 g of diborane?
(Atomic weight of B = 10.8 u)
oxygen released can completely burn 27.66 g of diborane?
(Atomic weight of B = 10.8 u)
MCQ+4 / -12018
31Electrochemistry
To find the standard potential of M3+/M electrode,the following cell is constituted : Pt/M/M3+(0.001 mol L−1 )/Ag+(0.01 mol L−1 )/Ag
The emf of the cell is found to be 0.421 volt at 298 K. The standard potential of half reaction M3+ + 3e−...
The emf of the cell is found to be 0.421 volt at 298 K. The standard potential of half reaction M3+ + 3e−...
MCQ+4 / -12017
32Electrochemistry
Consider the following standard electrode potentials (Eo in volts) in aqueous solution :
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MCQ+4 / -12017
33Electrochemistry
What is the standard reduction potential (Eo) for Fe3+ \(\to\) Fe ?
Given that :
Fe2+ + 2e\(-\) \(\to\) Fe; \(E_{F{e^{2 + }}/Fe}^o\) = \(-\)0.47 V
Fe3+ + e\(-\) \(\to\) Fe2+; \(E_{F{e^{3 + }}/F{e^{2 + }}}^o\) = +0.77 V
Given that :
Fe2+ + 2e\(-\) \(\to\) Fe; \(E_{F{e^{2 + }}/Fe}^o\) = \(-\)0.47 V
Fe3+ + e\(-\) \(\to\) Fe2+; \(E_{F{e^{3 + }}/F{e^{2 + }}}^o\) = +0.77 V
MCQ+4 / -12017
34Electrochemistry
Given
\(E_{C{l_2}/C{l^ - }}^o\) = 1.36 V, \(E_{C{r^{3 + }}/Cr}^o\) = - 0.74 V
\(E_{C{r_2}{O_7}^{2 - }/C{r^{3 + }}}^o\) = 1.33 V, \(E_{Mn{O_4}^ - /Mn ^{2+}}^o\) = 1.51 V
Among the following, the strongest reducing agent is :
\(E_{C{l_2}/C{l^ - }}^o\) = 1.36 V, \(E_{C{r^{3 + }}/Cr}^o\) = - 0.74 V
\(E_{C{r_2}{O_7}^{2 - }/C{r^{3 + }}}^o\) = 1.33 V, \(E_{Mn{O_4}^ - /Mn ^{2+}}^o\) = 1.51 V
Among the following, the strongest reducing agent is :
MCQ+4 / -12017