Electrochemistry NEET Previous Year Questions With Answers

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Electrochemistry NEET Previous Year Questions With Answers From 2006 to 2021. Pdf Download Link Also Given in this Post. Electrochemistry NEET MCQs with Answers

Explore popular questions from Class 12 Electrochemistry for NEET. This collection covers Electrochemistry previous 15 year NEET questions hand picked by experienced teachers.

Electrochemistry NEET Previous Year Questions

NEET- 2019

NEET 2019 Electrochemistry question

NEET -2019

neet 2019 electrochemistry question

NEET -2018

neet 2018 previous year question

NEET-2017
the electrochemical cell
Zn | ZnSO4 (0.01 M) || CuSO4(1.0M) | Cu, the emf of this Daniel cell is E1 When the concentration ZnSO4 is changed to 1.0 M and that of CuSO4 changed to 0.01 M, the emf changes to E2. From the followings, which one is the relationship between E1 and E2 ?
( Given, RTF=0.059)

  • (a) E1 = E2
  • (b) E1 < E2
  • (c) E1 > E2
  • (d) E2 = 0 ≠E1

NEET- 2016
The molar conductivity of a 0.5 mol/dm3 solution of AgNO3 with electrolytic conductivity of 5.76×10-3 S cm-1 at 298 K is

  • (a) 2.88 S cm2/mol
  • (b) 11.52 S cm2/mol
  • (c) 0.086 S cm2/mol
  • (d) 28.8 S cm2/mol

NEET- 2016
During the electrolysis of molten sodium chloride, the time required to produce 0.10 mol of chlorine gas using a current of 3 amperes is
(a) 55 minutes                        (b) 110 minutes
(c) 220 minutes                       (d) 330 minutes

NEET-2016
If the E°cell for a given reaction has a negative value, which of the following gives correct relationships for the values of ∆G° and Keq ?

  • (a) ∆G° >0;  Keq< 1
  • (b) ∆G° >0; Keq>1
  • (c) ∆G° < 0; Keq> 1
  • (d) ∆G° <0; Keq< 1

NEET- 2016
Zinc can be coated on iron to produce galvanised iron but the reverse is not possible. It is because
(a) zinc is lighter than iron
(b) zinc has lower melting point than iron
(c) zinc has lower negative electrode potential than iron
(d) zinc has higher negative electrode potential than iron

NEET-2016
The pressure of H2 required to make the potential of H2-electrode zero in pure water at 298 K is

  • 1. 10-12 atm
  • 2. 10-10 atm
  • 3. 10-4 atm
  • 4. 10-14 atm

NEET- 2016 The molar conductivity of a 0.5 mol/dm3 solution of AgNO3 with electrolytic conductivity of 5.76 x 10-3S cm-3 at 298 K is

  • 1.  11.5 cm2/mol
  • 2.  21.5 cm2/mol
  • 3.  31.5 cm2/mol
  • 4.  41.5 cm2/mol

NEET- 2015
A device that converts energy of combustion of fuels like hydrogen and methane, directly into electrical energy is known as
1. fuel cell
2. electrolytic cell
3. dynamo
4. Ni-Cd cell

NEET- 2014
The weight of silver (at. wt.= 108) displaced by a quantity of electricity which displaces 5600 mL of O2 at STP will be
1. 5.4g
2. 10.8g
3. 54.0g
4. 108.0g

AIPMT- 2014
When 0.1 mol is oxidised the quantity of electricity required to completely to is :
1. 96500 C
2. 2 x 96500 C
3. 9650 C
4. 96.50 C

NEET- 2013
A button cell used in watches functions as following

Zn(s) + Ag2O(s) + H2O (l) ⇌2Ag(s) + Zn2+(aq) + 2OH(aq)

If half cell potentials are

Zn2+aq + 2e- → Znx; Eo = -0.76VAg2Os + H2Ol + 2e- → 2Ags + 2OH-aq; Eo = 0.34V

The cell potential will be
1. 0.84 V
2. 1.34 V
3. 1.10 V
4. 0.42 V

NEET 2013
A hydrogen gas electrode is made by dipping platinum wire in a solution of HCl of pH = 10 and by passing hydrogen gas around the platinum wiere at one atm pressure. The oxidation potential of electrode would be?
1. 0.59 V
2. 0.118 V
3. 1.18 V
4. 0.059 V

NEET- 2013 At 25 ºC molar conductance of 0.1 molar aqueous solution of ammonium hydroxide is 9.54 ohm–1cm2 mol–1 and at infinite dilution its molar conductance is 238 ohm–1 cm2 mol–1. The degree or ionisation of ammonium hydroxide at the same concentration and temperature is :

1. 20.800%
2. 4.008%
3. 40.800%
4. 2.080%

NEET- 2013 A button cell used in watches functions as following 
Zn(s) + Ag2O(s) + H2O(l)  2Ag(s) + Zn2+ (aq) + 2OH (aq) 
If half cell potentials are : 
Zn2+ (aq) + 2e → Zn(s); E º = – 0.76 V 
Ag2O (s) + H2O (l) + 2e → 2Ag(s) + 2OH (aq); E º = 0.34 V 
The cell potential will be:
 
1. 0.42 V
 
2. 0.84 V
 
3. 1.34 V
 
4. 1.10 V

NEET- 2012
Limiting molar conductivity of NH4OH (i.e Åm(NH4OH)) is equal to:-

1. Åm (NH4Cl)+Åm(NaCl)-Åm(NaOH) 

2. Åm(NaOH)+Åm(NaCl)-Åm(NH4Cl)

3. Åm(NH4OH)+Åm(NH4Cl)-Åm(HCl)

4. Å(NH4Cl)+Å(NaOH)-Å(NaCl)

AIPMT- 2011
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
1. Y > X > Z
2. Z > X > Y
3. X > Y > Z
4. Y > Z > X

AIPMT- 2011 The electrode potentials for 

       Cu2+(aq)+e-→Cu+(aq)and Cu+(aq)+e-→Cu(s)
are +0.15 V and +0.50 V respectively. The value of ECu2+/Cu0will be (electrochemistry)
  • 1.  0.325 V
  • 2.  0.650 V
  • 3.  0.150V
  • 4.  0.500 V

AIPMT- 2011 Standard electrode potential for Sn4+/Sn2+ couple is +0.15 V and that for the Cr3+/Cr couple is -0.74. These two couple in their standard state are connected to make a cell. The cell potential will be

  • 1.  +0.89 V
  • 2.  +0.18 V
  • 3.  +1.83 V
  • 4.  +1.199 V

NEET- 2010 In producing chlorine by electrolysis 100 kW power at 125V is being consumed.How much chlorine per minute is liberated (ECE of chlorine is 0.367×10-6kgC-1)

  • (a) 1.76×10-3kg                                   (b) 9.67×10-3kg
  • (c) 17.61×10-3kg                                 (d) 3.67×10-3kg 

AIPMT -2011 For the reduction of silver ions with copper metal, the standard cell potential was found to be + 0.46 V a t 25 °C. The value of standard Gibbs energy, ΔGo will be (F = 96500C mol-1)

  • 1. -89.0 kJ
  • 2. -89.0 J
  • 3. -44.5 kJ
  • 4. -98.0 kJ

AIPMT- 2011 The electrode potentials for 

       Cu2+(aq)+e-→Cu+(aq)and Cu+(aq)+e-→Cu(s)
are +0.15 V and +0.50 V respectively. The value of ECu2+/Cu0will be (electrochemistry)
  • 1.  0.325 V
  • 2.  0.650 V
  • 3.  0.150V
  • 4.  0.500 V

AIPMT- 2010
An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to
1. increase in ionic moility of ions
2. 100% ionization of electrolyte at normal dilution
3. increase in both, i.e, number of ions and ionic mobility of ions
4. inrease in number of ions

AIPMT- 2010
For the reduction of silver ions with copper metal, the standard cell potential was found to be + 0.46 V a t 25 °C. The value of standard Gibbs energy, ΔGo will be (F = 96500C mol-1)
1. -89.0 kJ
2. -89.0 J
3. -44.5 kJ
4. -98.0 kJ

NEET- 2008
Kohlrausch’s law states that at
(a) finite dilution, each ion makes definite contribution to equivalent 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 depending on the nature of the other ion of th electrolyte
(c) infinite dilution, each ion makes definite contribution to 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, whatever be the nature of the other ion of the electrolyte

NEET- 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 E°cell for the pentane-oxygen fuel cell is

(a) 1.968 V

(b) 2.0968 V

(C) 1.0968 V

(d) 0.0968 V

NEET- 2007
The equilibrium constant of the reaction:

 Cu (s) + 2Ag+ (aq) →Cu2+ (aq) + 2Ag(s) ;

E° = 0.46 V at 298 K is:

(a) 2.4 x 1010              (b) 2.0 x 1010

(c) 4.0 x 1010              (d) 4.0 x 1015

NEET- 2007
The efficiency of a fuel cell is given by:
(a) ∆H/∆G     (b) ∆G/∆S    (c) ∆G/∆H    (d) ∆S/∆G

NEET- 2006
A hypothetical electrochemical cell is shown below AlA+ (xM)l l B+ (yM)l B+
The emf measured is +0.20V.The cell reaction is:-
(a) A++B→A+B+
(b) A++e→A;B++e→B
(c) the cell reaction cannot be predicted
(d) A+B+→A++B

AIPMT- 2006 If EFe2+/Feo = -0.441 V and 
EFe3+/Fe2+o = 0.771 V, the standard emf of the reaction : 
Fe + 2Fe3+→ 3Fe2+ will be :

  • 1. 0.330 V
  • 2. 1.653 V
  • 3. 1.212 V
  • 4. 0.111 V

AIPMT 2006 A hypothetical electrochemical cell is shown below A|A+ (xM) || B+ (yM)| B+ 
The emf measured is +0.20V. The cell reaction is :

  • 1. A++B→A+B+
  • 2. A++e-→A;B++e-→B
  • 3. the cell reaction cannot be predicted
  • 4. A+B+→A++B

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Class 12 Electrochemistry NEET Previous Year Questions with Answer is Here ! 


NEET Chemistry 12th C3 Electrochemistry Question
NEET 2020 to 1991



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