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Electrochemistry

75 Questions
All Exams NEET AIIMS
2011 NEET MCQ
AIPMT 2011 Prelims
Standard electrode potential of three metals X, Y and Z are $-$1.2 V, + 0.5 V and $-$ 3.0 V respectively. The reducing power of these metals will be
A.
Y > Z > X
B.
Y > X > Z
C.
Z > X > Y
D.
X > Y > Z
2010 NEET MCQ
AIPMT 2010 Mains
Which of the following expressions correctly represents the equivalent conductance at infinite diluation of Al2(SO4)3. Given that $\mathop \Lambda \limits^ \circ $Al3+ and $\mathop \Lambda \limits^ \circ $so$_4^{2 - }$ are the equivalent conductances at infinite dilution of the respective ions?
A.
$2\mathop \Lambda \limits^ \circ $Al3+   +   $3\mathop \Lambda \limits^ \circ $so$_4^{2 - }$
B.
$\mathop \Lambda \limits^ \circ $Al3+   +   $\mathop \Lambda \limits^ \circ $so$_4^{2 - }$
C.
($\mathop \Lambda \limits^ \circ $Al3+   +   $\mathop \Lambda \limits^ \circ $so$_4^{2 - }$) $ \times $ 6
D.
${1 \over 3}$$\mathop \Lambda \limits^ \circ $Al3+   +   ${1 \over 2}$$\mathop \Lambda \limits^ \circ $so$_4^{2 - }$
2010 NEET MCQ
AIPMT 2010 Mains
Consider the following relations for emf of an electrochemical cell
(i)   EMF of cell = (Oxidation potential of anode) $-$ (Reduction potential of cathode)
(ii)  EMF of cell = (Oxidation potential of anode) + (Reduction potential of cathode)
(iii) EMF of cell = (Reductional potential of anode) + (Reduction potential of cathode)
(iv) EMF of cell = (Oxidation potential of anode) $-$ (Oxidation potential of cathode)

Which of the above relations are correct?
A.
(iii) and (i)
B.
(i) and (ii)
C.
(iii) and (iv)
D.
(ii) and (iv)
2010 NEET MCQ
AIPMT 2010 Prelims
An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to
A.
increase in ionic mobility of ions
B.
100% ionisation of electrolyte at normal dilution
C.
increase in both i.e., number of ions and ionic mobility of ions
D.
increase in number of ions.
2010 NEET MCQ
AIPMT 2010 Prelims
For the reduction of silver ions with copper metal, the standard cell potential was found to be + 0.46 V at 25oC. The value of standard Gibb's energy, $\Delta $Go will be
(F = 96500 C mol$-$1)
A.
$-$ 89.0 kJ
B.
$-$ 89.0 J
C.
$-$ 44.5 kJ
D.
$-$ 98.0 kJ
2009 NEET MCQ
AIPMT 2009
The equivalent conductance of M/32 solution of a weak monobasic acid is 8.0 mho cm2 and at infinite dilution is 400 mho cm2. The dissociation constant of this acid is
A.
1.25 $ \times $ 10$-$6
B.
6.25 $ \times $ 10$-$4
C.
1.25 $ \times $ 10$-$4
D.
1.25 $ \times $ 10$-$5
2009 NEET MCQ
AIPMT 2009
Al2O3 is reduced by electrolysis at low potentials and high currents. If 4.0 $ \times $ 104 amperes of current is passed through molten Al2O3 for 6 hours, what mass of aluminium is product? (Assume 100% current efficiency, at mass of Al = 27 g mol$-$1).
A.
8.1 $ \times $ 104 g
B.
2.4 $ \times $ 105 g
C.
1.3 $ \times $ 104 g
D.
9.0 $ \times $ 103 g
2009 NEET MCQ
AIPMT 2009
Given :
(i)   Cu2+ + 2e$-$ $ \to $ Cu,  Eo = 0.337 V
(ii)  Cu2+ + e$-$ $ \to $ Cu+,  Eo = 0.153 V
Electrode potential, Eo for the reaction,
Cu+ + e$-$ $ \to $ Cu,  will be
A.
0.90 V
B.
0.30 V
C.
0.38 V
D.
0.52 V
2008 NEET MCQ
AIPMT 2008
On the basis of the following Eo values, the strongest oxidizing agent is
[Fe(CN)6]4$-$ $ \to $ [Fe(CN)6]3$-$ + e$-$;  Eo = $-$0.35 V

Fe2+ $ \to $ Fe3+ + e$-$;  Eo = $-$0.77 V
A.
Fe3+
B.
[Fe(CN)6]3$-$
C.
[Fe(CN)6]4$-$
D.
Fe2+
2008 NEET MCQ
AIPMT 2008
Kohlrausch's law states that at
A.
Infinite dilution, each ion makes definite contribution to conductance of an electrolyte whatever be the nature of the other ion of the electrolyte
B.
Infinite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte
C.
Finite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte
D.
Infinite dilution each ion makes definite contribution to equivalent conductance of an electrolyte depending on the nature of the other ion of the electrolyte.
2008 NEET MCQ
AIPMT 2008
Standard free energies of formation (in kJ/mol) at 298 K are $-$237.2, $-$ 394.4 and $-$8.2 for H2O(l), CO2(g) and pentane (g) respectively. The value of Eocell for the pentane-oxygen fuel cell is
A.
1.0968 V
B.
0.0968 V
C.
1.968 V
D.
2.0968 V
2007 NEET MCQ
AIPMT 2007
The equilibrium constant of the reaction:
Cu(s) + 2Ag+(aq) $ \to $ Cu2+(aq) + 2Ag(s);
Eo = 0.46 V at 298 K is
A.
2.0 $ \times $ 1010
B.
4.0 $ \times $ 1010
C.
4.0 $ \times $ 1015
D.
2.4 $ \times $ 1010
2007 NEET MCQ
AIPMT 2007
The efficiency of a fuel cell is given by
A.
$\Delta $G/$\Delta $S
B.
$\Delta $G/$\Delta $H
C.
$\Delta $S/$\Delta $G
D.
$\Delta $H/$\Delta $G
2006 NEET MCQ
AIPMT 2006
A hypothetical electrochemical cell is shown below.

$A\left| {{A^ + }\left( {xM} \right)} \right|\left| {{B^ + }\left( {yM} \right)} \right|B$

The emf measured is + 0.20 V. The cell reaction is
A.
A + B+ $ \to $ A+ + B
B.
A+ + B $ \to $ A + B+
C.
A+ + e$-$ $ \to $ A;  B+ + e$-$ $ \to $ B
D.
the cell reaction cannot be predicted.
2006 NEET MCQ
AIPMT 2006
EoFe2+/Fe = $-$ 0.441 V and EoFe3+/Fe2+ = 0.771 V, the standard EMF of the reaction Fe + 2Fe3+ $ \to $ 3Fe2+ will be
A.
0.111 V
B.
0.330 V
C.
1.653 V
D.
1.212 V
2005 NEET MCQ
AIPMT 2005
4.5 g of aluminium (at. mass 27 amu) is deposited at cathode from Al3+ solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from H ions in solution by the same quantity of electric charge will be
A.
44.8 L
B.
22.4 L
C.
11.2 L
D.
5.6 L
2005 NEET MCQ
AIPMT 2005
The mass of carbon anode consumed (giving only carbon dioxide) in the production of 270 kg of aluminium metal from bauxite by the Hall process is
(Atomic mass : Al = 27)
A.
270 kg
B.
540 kg.
C.
90 kg
D.
180 kg
2004 NEET MCQ
AIPMT 2004
The standard e.m.f. of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25oC. The equilibrium constant of the reaction would be
A.
2.0 $ \times $ 1011
B.
4.0 $ \times $ 1012
C.
1.0 $ \times $ 102
D.
1.0 $ \times $ 1010
2003 NEET MCQ
AIPMT 2003
The e.m.f. of a Daniell cell at 298 K is E1.
AIPMT 2003 Chemistry - Electrochemistry Question 29 English
When the concentration of ZnSO4 is 1.0 M and that of CuSO4 is 0.01 M, the e.m.f. changed to E2. What is the relationship between E1 and E2?
A.
E1 > E2
B.
E1 < E2
C.
E1 = E2
D.
E2 = 0 $ \ne $ E1
2003 NEET MCQ
AIPMT 2003
On the basis of the information available from the reaction,

4/3Al + O2 $ \to $ 2/3Al2O3,   $\Delta $G = $-$ 827 kJ mol$-$1 of O2,

the minimum e.m.f. required to carry out an electrolysis of Al2O3 is
(F = 96500 C mol$-$1)
A.
2.14 V
B.
4.28 V
C.
6.42 V
D.
8.56 V
2002 NEET MCQ
AIPMT 2002
In electrolysis of NaCl when Pt electrode is taken then H2 is liberated at cathode while with Hg cathode it forms sodium amalgam
A.
Hg is more inert than Pt
B.
More voltage is required to reduce H+ at Hg than at Pt
C.
Na is dissolved in Hg while it does not dissolve in Pt
D.
Conc. of H+ ions is larger when Pt electrode is taken.
2001 NEET MCQ
AIPMT 2001
Standard electrode potentials are
Fe2+/Fe [Eo = $-$0.44] and
Fe3+/Fe2+[ Eo = 0.77];
If Fe2+, Fe3+ and Fe blocks are kept together, then
A.
Fe3+ increases
B.
Fe3+ decreases
C.
Fe2+/Fe3+ remains unchanged
D.
Fe2+ decreases.
2000 NEET MCQ
AIPMT 2000
Cell reaction is spontaneous when
A.
$\Delta $Go is negative
B.
$\Delta $Go is positive
C.
$\Delta $Eored is positive
D.
$\Delta $Eored is negative
2000 NEET MCQ
AIPMT 2000
For the disproportionation of copper
2Cu+  $ \to $ Cu2+ + Cu, Eo is
(Given Eo for Cu2+/Cu is 0.34 V and
Eo for Cu2+/Cu+ is 0.15 V.)
A.
0.49 V
B.
$-$ 0.19 V
C.
0.38 V
D.
$-$0.38 V
2000 NEET MCQ
AIPMT 2000
Equivalent conductances of Ba2+ and Cl$-$ ions are 127 and 76 ohm$-$1 cm$-$1 eq$-$1 respectively. Equivalent conductance of BaCl2 at infinite dilution is
A.
139.5
B.
101.5
C.
203
D.
279