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Test: Electrochemistry - NEET MCQ


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30 Questions MCQ Test - Test: Electrochemistry

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Test: Electrochemistry - Question 1

           

The E° in the given diagram is,

Detailed Solution for Test: Electrochemistry - Question 1

∴   ΔG0= ΔG10 +ΔG20 + ΔG30

-6FE0. = -4F x 0.54 - 1F x 1.07

Test: Electrochemistry - Question 2

What is cell entropy change of the following cell?

Pt(s) | H2(g) | CH3COOH, HCl || KCl (aq) |Hg2Cl2| (s) | Hg

P = 1 atm        0.1M                0.1M

Emf of the cell is found to be 0.045 V at 298 K and temperature coefficient is 

3.4 x10–4  VK–1

Given Ka (CH3COOH) = 10–5 M

Detailed Solution for Test: Electrochemistry - Question 2

 

= 65.223J/K/mole

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Test: Electrochemistry - Question 3

Following cell has EMF 0.7995 V.

Pt | H2 (1 atm) | HNO3 (1M) || AgNO3 (1M) | Ag

If we add enough KCl to the Ag cell so that the final Cl- is 1M. Now the measured emf of the cell is 0.222 V.

The Ksp of AgCl would be :

Detailed Solution for Test: Electrochemistry - Question 3

Test: Electrochemistry - Question 4

The solubility of [Co(NH3)4Cl2] CIO4_________ if the  = 50,  = 70, and the measured resistance was 33.5Ω in a cell with cell constant of 0.20 is ____.

Detailed Solution for Test: Electrochemistry - Question 4

The correct answer is option B
Given,
λCo(NH3)4Cl2+=50       λClo-4 =70
λ∞= λCo(NH3)4Cl2+  + λClo-4
λ∞= 50             + 70
λ∞=120
(x) Cell constant = 1/A
0.02 = l/A
Resistance(R)   =33.5Ω
K =c.x              (x = is cell constant)

S  =49.7 mol/L

Test: Electrochemistry - Question 5

We have taken a saturated solution of AgBr.Ksp of AgBr is 12 x 10 – 14 . If 10 – 7 mole of AgNO3 are added to 1 litre of this solution then the conductivity of this solution in terms of  10 – 7 Sm – 1 units will be

[given  Sm2 mol-1 Smmol-1, 5 x 10-3 Sm2mol-1]

Detailed Solution for Test: Electrochemistry - Question 5

The solubility of Agbr in presence of 10-7 molar AgNo3 is 3 x 10-7 M. therefore [Br] 3 x 10-4 M3, [Ag+] = 4 x 10-4 m3 and [No3-]= 10-4 m3

Therefore 

Test: Electrochemistry - Question 6

At 298K the standard free energy of formation of H2O(L) is – 237.20kJ/mole while that of its ionisation into H+ ion and hydroxyl ions is 80 kJ/mole, then the emf of the following cell at 298 K will be

 H2(g,1 bar) | H+ (1M) || OH (1M) | O2 (g, 1bar)

Detailed Solution for Test: Electrochemistry - Question 6

Cell reaction

also we have

Hence for cell reaction

Test: Electrochemistry - Question 7

Which of the following cell can produce more electric work.

Detailed Solution for Test: Electrochemistry - Question 7

For Ecell to be highest [H+]a should be lower and [H+]c should be higher and that why anode compartment should be more basic and cathodic compartment should be acidic. 

Test: Electrochemistry - Question 8

A hydrogen electrodes is immersed in a solution with pH = 0 (HCl). By how much will the potential (reduction) change if an equivalent amount of NaOH is added to the solution. (Take PH2 = 1 atm) T = 298 K.

Detailed Solution for Test: Electrochemistry - Question 8

pH changes from 0 to 7

∴ [H+] changes from 1 to 10-7 M

Accordingly Ered. Decrease by 0.059 log 10-7 i.e 0.059 x (-7) = -0.41volt

Test: Electrochemistry - Question 9

At what  does the following cell have its reaction at equilibrium?

 Ag(s) | Ag2CO3(s) | Na2CO3 (aq) || KBr(aq) | AgBr(s) | Ag(s)

 KSP =  8 x 10 – 12 for  Ag2CO3 and KSP = 4 x 10 – 13 for AgBr

Detailed Solution for Test: Electrochemistry - Question 9

Test: Electrochemistry - Question 10

Calculate the EMF of the cell at 298 K

Pt|H2(1atm)|NaOH(xM),NaCl(xM)|AgCl(s)|Ag

If E°cl-/AgCl/Ag = + 0.222 V

Detailed Solution for Test: Electrochemistry - Question 10

Test: Electrochemistry - Question 11

A current of 0.1A was passed for 2hr through a solution cuprocyanide and 0.3745g f copper was deposited on the cathode. Calculate the current efficiency for the copper deposition.

Detailed Solution for Test: Electrochemistry - Question 11

Test: Electrochemistry - Question 12

With t taken in seconds and I taken in Amp, the variation of I follows the equation

 t2 + I2 = 25

what amount of Ag will be electrodeposited with this current flowing in the interval 0-5 second ? (Ag : 108)

Detailed Solution for Test: Electrochemistry - Question 12

 

=21.97mg = 22mg

Test: Electrochemistry - Question 13

A resistance of 50Ω is registered when two electrodes are suspended into a beaker containing a dilute solution of a strong electrolyte such that exactly half of the them are submerged into solution. If the solution is diluted by adding pure water (negligible conductivity) so as to just completely submerge the electrodes, the new resistance offered by the solution would be

Detailed Solution for Test: Electrochemistry - Question 13

the k is halved while the A is doubled. Hence R remain 50 Ω.

Test: Electrochemistry - Question 14

The standard reduction potential of a silver chloride electrode is 0.2 V and that of a silver electrode is 0.79 V. The maximum amount of AgCl that can dissolve in 106 L of a 0.1 M AgNO3 solution is          

Detailed Solution for Test: Electrochemistry - Question 14

Test: Electrochemistry - Question 15

Calculate the cell EMF in mV for

Pt|H2(1atm) |HCl(0.01M)|AgCl(s)| Ag(s)        at 298 K

 If ΔG°r values are at 25°C

  for AgCl(s) and  for H+ + Cl-) (aq)

Detailed Solution for Test: Electrochemistry - Question 15

Test: Electrochemistry - Question 16

Adiponitrile is manufactured electrolytically from acrylonitrile

 CH2 = CHCN → CN – (CH2)4 – CN

How many kg of adiponitrile (molecular mass = 108) is produced in 9.65 hr using a current of 3750 A with 80% efficiency

Detailed Solution for Test: Electrochemistry - Question 16

Test: Electrochemistry - Question 17

It is observed that the voltage of a galvanic cell using the reaction M(s) + xH+→ Mx+ + X/2H2 varies linearly with the log of the square root of the hydrogen pressure and the cube root of the Mx+ concentration. The value of x is       

Detailed Solution for Test: Electrochemistry - Question 17

Test: Electrochemistry - Question 18

Acetic acid has Ka = 1.8 X 10 – 5 while formic acid had Ka = 2.1 X 10–4. What would be the magnitude of the emf of the cell

Detailed Solution for Test: Electrochemistry - Question 18

Test: Electrochemistry - Question 19

Consider the cell Ag(s)|AgBr(s)|Br-(aq)||AgCl(s)|Cl-(aq)|Ag(s) at 25°C. The solubility product constants of AgBr & AgCl are respectively 5 X 10 – 13 & 1 X 10 – 10. For what ratio of the concentrations of Br- & Cl- ions would the emf of the cell be zero ?           

Detailed Solution for Test: Electrochemistry - Question 19

Test: Electrochemistry - Question 20

Value of  for SrCl2 in water at 25°C from the following data:

Detailed Solution for Test: Electrochemistry - Question 20

Test: Electrochemistry - Question 21

Calculate the useful work of the reaction Ag(s) + 1/2Cl2(g) → AgCl(s)
Given  E°cl2/cl- = + 1.36 V,       E°AgCl/Ag,Cl- = 0.22 V

If         Pcl2 = 1 atm     and T = 298 K

Detailed Solution for Test: Electrochemistry - Question 21

(1) AgCl (s) + e → Ag(s) + Cl-         E0 = 22 V

(2) 1/2 Cl2 + e → Cl-             E= 1.36V

we get

Ag(s) + 1/2Cl2 (g) →AgCl(s)          E0cell = 1.14V

Test: Electrochemistry - Question 22

Which of these ions Cu+, Co3+, Fe2+ is stable in aqueous medium.

Given :

Cu2+/Cu+ = 0.15 volt ;            E°Cu+/Cu = 0.53 V ;       E°Co3+/Co2+ = 1.82 V ;

Fe3+/Fe2+ = 0.77 V ;   E°Fe2+Fe = - 0.44 V ;    E°O2,H+/H2O = 1.23 V

Detailed Solution for Test: Electrochemistry - Question 22

 if reduction potential of metal ion is greater then O2/H2O couple, the ion is stable in water. So Co3+ is stable in water

Test: Electrochemistry - Question 23

Select the correct statement if -

Mg2+/Mg = - 2.4V,      E°Sn4+/Sn2+ = 0.1 V,     E°MnO4-,H+/Mn2+ = 1.5 V, E° I2/I- = 0.5 V    Here,

Detailed Solution for Test: Electrochemistry - Question 23

[Hint: Reverse of (B) & (C) is spontaneous; weakest Oxidizing Agent here is Mg2+]

Test: Electrochemistry - Question 24

 What is the value of pKb (CH3COOH-) if λm = 390 & λm = 7.8 for 0.04 of a CH3COOH at 25°C          

Detailed Solution for Test: Electrochemistry - Question 24

Test: Electrochemistry - Question 25

The temperature coefficient of a standard Cd-cell is – 5.0X10– 5 Vk– 1 whose emf at 25°C is 1.018 V. During the cell operation, the temperature will -           

Detailed Solution for Test: Electrochemistry - Question 25

Test: Electrochemistry - Question 26

 A cell Ag | Ag+ || Cu++ | Cu initially contains 2M Ag+ and 2M Cu++ ions. The charger in cell potential after the passage of 10 amp current for 4825 sec is:          

Detailed Solution for Test: Electrochemistry - Question 26

Test: Electrochemistry - Question 27

For the cell (at 298 K)

Ag(s) | AgCl(s) | Cl-(aq) || AgNO3(aq) | Ag(s)

Which of the following is correct –

Detailed Solution for Test: Electrochemistry - Question 27

Conductivity is high due to [H+]

Test: Electrochemistry - Question 28

During an electrolysis of conc. H2SO4, perdissulphuric acid (H2S2O8) and O2 from in equimolar amount. The amount of H2 that will form simultaneously will be (2H2SO4 → H2S2O8 + 2H+ + 2e-)

Detailed Solution for Test: Electrochemistry - Question 28

Test: Electrochemistry - Question 29

Statement-1: In electrochemical cell, we cannot use KCI in the salt bridge if anodic  or cathodic compartment consists of Ag+ of Pb2+ ion.

Statement-2: Salt bridge is employed to maintain the electrical neutrality and to minimize the liquid-liquid junction potential.

Detailed Solution for Test: Electrochemistry - Question 29

Both (S – 1) & (S – 2) are true and (S – 2) is not the correct explanation of    (S – 1)

Test: Electrochemistry - Question 30

Statement-1: Zinc protect the iron better than tin even after it cracks.

Statement-2:OPzn < E°OPfe But E°OPSn > E°OPfe

Detailed Solution for Test: Electrochemistry - Question 30

The correct answer C
EZn+2∣Zn  < EFe+2∣Fe<E+2Sn∣Sn
   SPR ↓  Reactivity ↑

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