MCQ Questions Chapter 3 Electrochemistry Class 12 Chemistry

Please refer to MCQ Questions Chapter 3 Electrochemistry Class 12 Chemistry with answers provided below. These multiple-choice questions have been developed based on the latest NCERT book for class 12 Chemistry issued for the current academic year. We have provided MCQ Questions for Class 12 Chemistry for all chapters on our website. Students should learn the objective based questions for Chapter 3 Electrochemistry in Class 12 Chemistry provided below to get more marks in exams.

Chapter 3 Electrochemistry MCQ Questions

Please refer to the following Chapter 3 Electrochemistry MCQ Questions Class 12 Chemistry with solutions for all important topics in the chapter.

MCQ Questions Answers for Chapter 3 Electrochemistry Class 12 Chemistry

Question. The standard reduction potential values of the three metallic cations X,Y and Z are 0.52, −3.03 and −1.18 V respectively. The order of reducing power of the corresponding metals is
(a) Y > Z > X
(b) X > Y > Z
(c) Z > Y > X   
(d) Z > X > Y         

Question. Given, E° _{Cl /Cl}− = 1.36 V;E ° _Cr3+ = −  /Cr 0.74 V
         E° _Cr2O27/Cr3+ =1.33 V;E ° _{MnO4- /Mn²⁺} = 1.51V
Among the following, the strongest reducing agent is
(a) Cr
(b) Mn²⁺
(c) Cr³⁺
(d) Cl−             

Question. Conductance (unit Siemen’s) is directly proportional to area of the vessel and the concentration of the solution in it and is inversely proportional to the length of the vessel, then the unit of constant of proportionality is
(a) S m mol^–1
(b) S m² mol ^–1
(c) S^–2 m² mol  
(d) S² m² mol^–2           

Question. Resistance of 0.2 M solution of an electrolyte is 50 W. The specific conductance of the solution is 1.3 S m⁻¹. If resistance of the 0.4 M solution of the same electrolyte is 260 , its molar conductivity is 
(a) 6250 Sm² mol⁻¹
(b) 6.25 × 10⁻⁴ Sm² mol⁻¹
(c) 625 × 10⁻⁴ Sm² mol⁻¹
(d) 62.5 Scm² mol⁻¹         

Question. A solution of copper sulphate (CuSO₄ ) is electrolysed for 10 min with a current of 1.5 A. The mass of copper deposited at the cathode (Atomic mass of Cu = 63u ) is 
(a) 0.3892 g
(b) 0.2938 g
(c) 0.2398 g
(d) 0.3928 g               

Question. Resistance of 0.2 M solution of an electrolyte is 50 W. The specific conductance of the solution of 0.5 M solution of same electrolyte is 1.4 Sm⁻¹ and resistance of same solution of the same electrolyte is 280 .The molar conductivity of 0.5Msolution of the electrolyte in Sm₂ mol⁻¹ is
(a) 5 × 10⁻⁴
(b) 5 × 10⁻³
(c) 5 × 10³
(d) 5 × 10²         

Question. The equivalent conductance of NaCl at concentration (C) and at infinite dilution are λ_C and λ_∞,respectively. The correct relationship betweenλ_C and λ_∞ is given as (Where, the constant B is positive) 
(a) λ_C = λ_∞ + (B)C
(b) λ_C = λ_∞ − (B)C
(c) λ_C = λ_∞ − (B)√C
(d) λ_C = λ_∞ + (B)√C         

Question. X g of silver is plated out on a serving tray by electrolysis of a solution containing silver in +1 oxidation state for a period of 8.0 h at a current of 8.46 A. What is the area of the tray if the thickness of silver plating is 0.00254 cm?
[Given, density of silver = 10.5 g cm⁻³]
(a) 10.7 × 10⁴ cm²
(b) 1.02 × 10⁴ cm²
(c) 4.1 × 10³ cm²
(d) 10.2 × 10⁴ cm²           

Question. A current of 2 A is passed for 5 h through a molten tin salt to deposit 22.2 g tin. What is the oxidation state of tin in salt ? [At. wt. of Sn =118.69 g]
(a) +2
(b) +5
(c) +3
(d) +4             

Question. For the reaction,
    Zn(s) + Cu²+ (0.1 M) → Zn²⁺ (1M) + Cu(s)
taking place in a cell, E°_cell o is 1.10 V. E°_cell for the cell will be{2.303 RT/F =0.0591}
(a) 1.80 V
(b) 1.07 V
(c) 0.82 V
(d) 2.14 V                     

Question. Given, E°_Cr3+/Cr = −0.72 V; E° _Fe2+/Fe 0.42 V o = −
The potential for the cell
       Cr|Cr³⁺ (0.1M)||Fe²⁺ (0.01M) |Fe is
(a) − 0.339 V
(b) − 0.26 V
(c) 0.26 V
(d) 0.339 V         

Question. In the electrolytic cell, flow of electrons is from
(a) cathode to anode in solution
(b) cathode to anode through external supply
(c) cathode to anode through internal supply
(d) anode to cathode through internal supply             

Question. When the sample of copper with the zinc impurity is to be purified by electrolysis, the appropriate electrodes are
      Cathode             Anode
(a) pure zinc         pure copper
(b) impure zinc     pure copper
(c) impure zinc     impure sample
(d) pure copper    impure sample               

Question. The value of the reaction quotient, Q for the cell Zn (s)| Zn²⁺(0.01M)| | Ag⁺ (1.25 M)| Ag(s) is
(a) 156
(b) 125
(c) 1.25 × 10^–2
(d) 6.4 × 10^–3           

Question. The reduction potential of hydrogen half-cell will be negative if 
(a) p (H₂ ) = 1 atm and|H+| = 2.0 M
(b) p (H₂ ) = 1 atm and|H+| = 1.0 M
(c) p (H₂ ) = 1 atm and|H+| = 1.0 M
(d) p (H₂ ) = 1 atm and|H+| = 2.0 M           

Question. The standard reduction potential for Fe Fe²⁺ / and Sn Sn²⁺ / electrodes are – 0.44 and – 0.14 V respectively. For the cell reaction; Fe²⁺ + Sn → Fe + Sn²⁺ , the standard emf is
(a) +0.30 V
(b) – 0.58 V
(c) +0.58 V
(d) – 0.30 V         

Question. How many Faraday’s are required to reduce 1 mole of BrO₃^– to Br –?
(a) 3
(b) 5
(c) 6
(d) 4               

Question. Two Faraday of electricity is passed through a solution of CuSO₄.The mass of copper deposited at the cathode is (atomic mass Cu = 63.5u) 
(a) 0 g
(b) 63.5 g
(c) 2 g
(d) 127 g             

Question. What will be the emf for the given cell?
     Pt | H₂(p₁) | H⁺ (aq) | H₂(p₂ ) | Pt
(a) RT/F ln p₁/p₂
(b) RT/2F ln p₁/p₂
(c) RT/2F ln p₂/p₁
(d) None of these             

Question. The metal that cannot be obtained by electrolysis of an aqueous solution of its salts is 
(a) Ag
(b) Ca
(c) Cu
(d) Cr       

Question. Given, E° _{Cr3+ /Cr} = −0.74 V;E° _{MnO4- /Mn²⁺} = 1.51V
         E° _Cr2O2-/Cr3+ =1.33 V;E ° _{Cl /Cl}−=1.33 V
Based on the data given above, strongest oxidising agent will be 
(a) Cr³⁺
(b) Mn²⁺
(c) MnO₄⁻
(d) Cl⁻                     

Question. Electrode potentials (E °) are given below :
        Cu+ / Cu = + 0.52 V, Fe³⁺/Fe²⁺ =+0.77 V
       1/2 I₂(s) / I^{− =+} 0.54V, Ag⁺ /Ag = + 0.88 V
Based on the above potentials strongest oxidising agent will be 
(a) Cu
(b) Fe³⁺
(c) Ag⁺
(d) I₂           

Question. In the cell reaction,
Cu(s) + 2Ag⁺ (aq)→ Cu²⁺ (aq) + 2Ag(s),E°_cell  = 0.46 V by doubling the concentration of Cu²⁺ , E_cell is
(a) doubled
(b) halved
(c) increased but less than double
(d) decreased by a small fraction               

Question. For a saturated solution of AgCl at 25°C, specific conductance is 3.41 ×10⁻⁶ omh^–1 cm^–1 and that water used for preparing the solution was
1.60×10⁻⁶ ohm–¹ cm^–1 The solubility product of AgCl is [L^∞_eqAgCl) =138.3 ohm^–1 cm^–1 equiv^–1]
(a) 1.31 × 10⁻⁵
(b) 1.74 × 10⁻⁸
(c) 1.72 × 10⁻¹⁰
(d) 3.61 × 10⁻³             

Question. The ionic conductance of Ba²⁺ and Cl^– are respectively 127 and 76 Ω^– cm² as infinite dilution. The equivalent conductance (in Ω^-1 cm²) of BaCl₂ at infinite dilution will be 
(a) 330
(b) 203
(c) 139.5
(d) 51     

Question. AgNO₃ (aq) was added to an aqueous KC! solution gradually and the conductivity of the solution was measured. The plot of conductance (A) versus the volume of AgNO₃ is

(a) (I)
(b) (II)
(c) (III)
(d) (IV)     

Question. Resistance of 0.2 M solution of an electrolyte is 50 Ω. The specific conductance of the solution is 1.3 sm^-1 . If resistance of the 0.4 M solution of the same electrolyte is 260 Ω, its molar conductivity is 
(a) 6250 Sm² mol^-1
(b) 6.25 x 10^-4 Sm² mol^-1
(c) 625 x 10^-4 Sm² mol^-1
(d) 62.5 Sm² mol^-1       

Question. The resistance of IN solution of acetic acid is 250Ω, when measured in a cell having a cell constant of 1.15 cm^-1. The equivalent conduction (in ohm^-1 cm² equiv^-1) of IN acetic acid is
(a) 2.3
(b) 4.6
(c) 9.2
(d) 18.4       

Question. The one which decreases with dilution is 
(a) molar conductance
(b) conductance
(c) specific conductance
(d) equivalent conductance       

Question. By diluting a weak electrolyte, specific conductivity (K_c) and equivalent conductivity (λ_c ) change as
(a) Both increase 
(b) K_c increases, λ_c  decreases
(c) K_c decreases, λ_c  increases
(d) Both decrease     

Question. Given the limiting molar conductivity as
^∧0_m(HCI) = 425. 9 Ω^-1 cm² mol^-1
∧0_m(NaCl)= 126.4 Ω^-1 cm² mol^-1
∧0_m(CH₃COONa) = 91 Ω^-1 cm² mol^-1
The molar conductivity, at infinite dilution, of acetic acid (in Ω^-1 cm² mol^-1) will be 
(a) 481.5
(b) 390.5
(c) 299.5
(d) 516.9     

Question. The molar conductivities of KCl, NaCl and KNO₃ are 152, 128 and 111 S cm² mol^-1 respectively. What is the molar conductivity of NaNO₃? 
(a) 101 cm² mol^-1
(b) 87 cm² mol^-1
(c) – 101 cm² mol^-1
(d) – 391 cm² mol^-1       

Question. Which one of the following solutions will have highest conductivity? 
(a) 0.1 M CH₃COOH
(b) 0.1 M NaCl
(c) 0.1 M KNO₃
(d) 0.1 M HCl     

Question. Which of the following electrolytic solutions has the least specific conductance?
(a) 0.02 N
(b) 0.2 N
(c) 2 N
(d) 0.002 N     

Question. The resistance of N/10 solution is found to be 2.5 x 10³ Ω. The equivalent conductance of the solution is ( cell constant = 1.25 cm^-1 ) 
(a) 2.5 Ω^-1 cm² equiv^-1
(b) 5. Ω^-1 cm² equiv^-1
(c) 2.5 Ω^-1 cm^-2 equiv^-1
(d) 5.0 Ω^-1 cm^-2 equiv^-1     

Question. The value of A^∞_eq for NH₄Cl, NaOH and NaCl are respectively, 149.74, 248.1 and 126.4 Ω^-1 cm^-2 equiv^-1 . The value of A^∞_eqof NH₄OH is
(a) 371.44
(b) 271.44
(c) 71.44
(d) Cannot be predicted from given data     

Question. Which of the following is not true?
(a) Cathode is negative terminal in an electrolytic cell
(b) Anode is positive terminal in a galvanic cell
(c) Reduction occurs at cathode in either of cells
(d) Oxidation occurs at anode                 

Question. Which of the following statement is correct?
(a) E_cell and Δ_rG of cell reaction both are extensive properties
(b) E_cell and Δ_rG of cell reaction both are intensive properties
(c) E_cell is an intensive property while Δ_rGof cell reaction is an extensive property
(d) E_cell is an extensive property while Δ_rG of cell reaction is an intensive property         

Question. The standard emf of a cell, involving one electron change is found to be 0.591V at 25°C. The equilibrium constant of the reaction is(1F = 96500 Cmol–1)
(a) 1.0 × 10¹
(b) 1.0 × 10⁵
(c) 1.0 × 10¹⁰
(d) 1.0 × 10³⁰           

Question. A gas X at 1 atm is bubbled through a solution containing a mixture of 1 MY_– and 1 MZ^– at 25°C. If the order of reduction potentials is Z > Y > X, then
(a) Y will oxidise X and not Z
(b) Y will oxidise Z and not X
(c) Y will oxidise both X and Y
(d) Y will reduce both X and Y               

Question. Given, E °_Fe3+ /Fe = − 0.036 V, E °_Fe²⁺ /Fe = −0.439 V
The value of standard electrode potential for the charge,
Fe³⁺(aq) + e− →Fe²⁺ (aq) will be
(a) – 0.072 V
(b) 0.385 V
(c) 0.770 V
(d) – 0.270 V                 

Question. Given below are the half-cell reactions
       Mn²⁺ + 2⁻_e → Mn ;E° 1.18eV 
      2(Mn³⁺ +⁻_e → Mn²⁺ ); E ° = + 1.51 eV 
      The  ° for 3Mn²⁺ → Mn + 2Mn³⁺ will be
(a) −2.69V; the reaction will not occur
(b) −2.69V; the reaction will occur
(c) −0.33 V; the reaction will not occur
(d) −0.33 V; the reaction will occur             

Question. Of the following metals that cannot be obtained by electrolysis of the aqueous solution of their salts are
(a) Ag and Mg
(b) Ag and Al
(c) Mg and Al
(d) Cu and Cr           

Question. The standard reduction potentials for Zn²⁺ / Zn, Ni²⁺ / Ni  and Fe²⁺ /Fe are − 0.76, − 0.23 and − 0.44 V respectively. The reaction X + Y ²⁺ → X ²⁺ + Y will be spontaneous when
(a) X = Ni,Y = Fe
(b) X = Ni,Y = Zn
(c) X = Fe,Y = Zn
(d) X = Zn,Y = Ni           

Question. Same quantity of charge is being used to liberate iodine (at anode) and a metalM (at cathode). The mass of metalM liberated is 0.617 g and the liberated iodine is completely reduced by 46.3 mL of 0.124 M sodium thiosulphate. What is the total time to bring this change if 10 A current is passed through solution of metal iodide?
(a) 55.4 s
(b) 25.2 s
(c) 5.54 s
(d) 16.8 s                 

Question. Galvanisation is applying a coating of 
(a) Cr
(b) Cu
(c) Zn  
(d) Pb             

Question. Aluminium oxide may be electrolysed at 1000°C to furnish aluminium metal
(Atomic mass = 27u; 1F = 96500 C).
The cathode reaction is Al³⁺ + 3e^– → Al.
To prepare 5.12 kg of aluminium metal by this method required electricity will be
(a) 5.49 × 10¹C
(b) 5.49 ×  10⁴C
(c) 1.83 × 10⁷C
(d) 5.49 × 10⁷C               

Question. How long (approximate) should water be electrolysed by passing through 100 A current so that the oxygen released can completely burn 27.66 g of diborane? (Atomic weight of B =10 8 . μ) 
(a) 6.4 h
(b) 0.8 h
(c) 3.2 h
(d) 1.6 h             

Question. Given the data at 25°C,
                        Ag + I⁻ → AgI +e⁻; E ° = 0.152 V
                       Ag Ag⁺ → + e⁻; E ° = − 0.800 V
What is the value of log K_sp for AgI ?
{2.303 RT/F = 0.059 V}
(a) − 8.12
(b) + 8.612
(c) −37.83
(d) −16.14             

Question. The Edison storage cell is represented as
    Fe(s)|FeO(s)|KOH(aq)| Ni2O3(s)|NiO(s)|Ni (s)
the half-cell reactions are
Ni₂O₃(s)+H₂O(l )+ 2e⁻ ⇌ 2NiO(s)+ 2OH⁻; 
FeO(s)+H₂O(l )+2e⁻ ⇌ e(s)+ 2OH−; eF E ° =− 0.87V
What is the maximum amount of electrical energy that can be obtained from one mole of Ni₂O₃?
(a) 127 kJ
(b) 245.11 kJ
(c) 90.71 kJ
(d) 122.55 kJ               

Question. The standard oxidation potentials of Zn, Cu, Ag and Ni electrodes are + 0.76, – 0. 34, – 0. 80 and + 0. 25 V respectively. Which of the following reaction will provide maximun1 voltage?
(a) Cu + 2Ag⁺ (aq) ➔ Cu²⁺ (aq) + 2Ag
(b) Zn + 2Ag⁺ (aq) ➔ Zn²⁺ (aq) + 2Ag
(c) H₂ + Ni²⁺ (aq) ➔ 2H⁺ (aq) + Ni
(d) Zn + Cu²⁺ (aq) ➔ Zn²⁺ (aq) + Cu
(e) Zn + 2H⁺ (aq) ➔ Zn²⁺ (aq) + H₂

Question. The standard emf of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25C° . The equilibrium constant of the reaction would be
(Given, F = 96500Cmol^-1, R = 8.3 14 JK^-1 mol^-1)
(a) 2.0 X 10¹¹
(b) 4.0 X 10¹² 
(c) 1.0 x 10²
(d) 1.0 x 10¹⁰

Question. The cell reaction of a cell is
Mg(s) + Cu²⁺ (aq) ➔ Cu (s) + Mg²⁺ (aq). If the standard reduction potentials of Mg and Cu are – 2. 37 and + 0. 34 V respectively. The emf of the cell is 
(a) 2.03 V
(b) – 2.03 V
(c) + 2.71 V
(d) – 2.71 V

Question. EMF of hydrogen electrode in te1m of pH is ( at 1 atrn pressure) 
(a) EH₂ = RT/F x pH
(b) EH₂ =RT/F.1/pH
(c) EH₂ = 2.303 RT/F.pH
(d) EH₂ = 0.0591 pH

Question. For the redox reaction,
Zn(s) + Cu²⁺ (0.1 M) ➔ Zn^z+ (1 M) + Cu(s)
taking place in a cell, E°_cell is 1.10 V. E°_cell for the cell willbe ( 2.303 RT/F = 0.0591) 
(a) 2.14 V
(b) 1.80 V
(c) 1.07 V
(d) 0.82 V

Question. Sn⁴⁺ + 2e^– ➔ Sn²⁺, E° = 0. 13 V
Br₂ + 2e^– ➔ 2Br^– ,E° = 1 .08V
Calculate K eq for the cell reaction for the cell formed by two electrodes. 
(a) 10⁴¹
(b) 10³²
(c) 10^-32
(d) 10^-42

Question. Calculate the emf of the cell
Cu(s) l Cu^z+ (aq) ll Ag⁺ (aq ) l Ag(s)
Given, E°_Cu2+/Cu = + 0.34 V, E°_{Ag⁺ /Ag} = 0.80 V
(a) + 0.46 V
(b) + 1.14 V 
(c) +0.57 V
(d) -0.46 V   

Question. The standard electrode potential of hydrogen electrode at 1 M concentration and hydrogen gas at 1 atrn pressure is
(a) 1 V
(b) 6 V 
(c) 8 V
(d) 0 V   

Question. 2Fe³⁺ + 3I^– ⇌ 2Fe²⁺ + I^–₃
The standard reduction potentials in acidic conditions are 0.77 and 0.54V respectively for Fe³⁺ / Fe²⁺ and I^–₃/ I^– rcouples. The equilibrium constant for the reaction is
(a) 6.26 X 10^-7
(b) 5.33 X 10^-4
(c) 6.26 x 1⁰⁷
(d) 5.33 x 10⁴   

Question. Which one of the following nitrates will leave behind a metal on strong heating?
(a) Ferric nitrate
(b) Copper nitrate
(c) Manganese nitrate
(d) Silver nitrate   

Question. An alloy of Pb-Ag weighing 1.08 g was dissolved in dilute HNO₃ and the volume made to 100 mL. A silver electrode was dipped in the solution and the emf of the cell set-up Pt(s ), H₂ (g) l H⁺ (l M) ll Ag⁺ (aq) l Ag(s) was 0.62 V. If E°_cell = 0. 80V, what is the percentage of Ag in the alloy? (At 25°C, RT/F = 0. 06) 
(a) 25
(b) 2.50
(c) 10
(d) 1
(e) 50

Question. In the electrochemical reaction,
2Fe³⁺ + Zn ➔ Zn²⁺ + 2Fe²⁺
increasing the concentration of Fe²⁺ 
(a) increases cell emf
(b) increases the current flow
(c) decreases the cell emf
(d) alter the pH of the solution

Question. Given the data at 25°C,
Ag + I^– ➔ AgI + e^– ;E° =0. 152 V
Ag ➔ Ag⁺ + e- ; E° = – 0. 800 V
What is the value of log K_sp for AgI?
( 2.303RT/F = 0.059 V)
(a) – 8.12
(b) +8.612
(c) – 37.83
(d) -16.13

Question. An inaccurate ammeter and silver coulometer is connected in series in an electric circuit through which a constant direct current flows. If ammeter reads 0.6 ampere throughout one hour, the silver deposited on coulometer was found to be 2.16 g. What per cent error is in the reading of ammeter ? [Assume 100% current efficiency].
(a) 1%
(b) 0.54%
(c) 0.06 %  
(d) 10%                     

Question.  An aqueous solution ofNaCl on electrolysis gives H₂₍g),Cl₂(g) and NaOH. According to reaction,
 2Cl⁻(aq)+ 2H₂O → 2OH⁻ (aq)+H₂(g) + Cl₂(g)
A direct current of 25 A with a current efficiency of 62% is passed through 20 L of NaCl solution (20% by weight). How long it take to produce 1 kg of Cl2?
(a) 30.20 h
(b) 12.17 h
(c) 48.71 h
(d) 14.61 h               

Question.  Zn|Zn²⁺ (a = 0.1 M)||Fe²⁺ (a = 0.01 M)|Fe.
The emf of the above cell is 0.2905 V.
Equilibrium constant for the cell reaction is
(a) 10 ^{0.32/ 0.0591}
(b) 10 ^{0.32/ 0.0295}
(c) 10 ^{0.26/ 0.0295}
(d) 10 ^{0.32/ 0.295}             

Question. The standard reduction potentials at 298 K for the following half reactions are given against each.
         Zn²⁺ (aq) + 2e^– ⇌ Zn(s); – 0.762 V
         Cr³⁺ (aq) + 3e^– ⇌ Cr(s); – 0.740 V
        2H⁺ (aq  + 2e^{– ⇌} H²(g); 0.00 V
        Fe³⁺ (aq) + e^– ⇌ Fe²⁺  2+ (aq); 0.770
Which is the strongest reducing agent?
(a) Zn (s)
(b) Cs (s)
(c) H₂ (g)
(d) Fe³⁺ (aq)                 

Question. The equivalent conductances of two strong electrolytes at infinite dilution inH O 2 (where ions move freely through a solution) at 25°C are given below
Λ° = CH₃COONa = 91.0 S cm² /equiv
Λ° _HCl = l 2 426.2 S cm² /equiv
What additional information/quantity one needs to calculate Λ° of an aqueous solution of acetic acid ?
(a) Λ° of NaCl
(b) Λ° of CH₃COK 
(c) The limiting equivalent conductance of H⁺ [λ° _H+ ]
(d) Λ° of chloroacetic acid (ClC_H2COOH)             

Question.  The rusting of iron takes place as follows:
      2H⁺ + 2e⁻ + 1/2 O₂  → H₂O (l);E °=+1.23 V
            Fe²⁺ + 2^–e → Fe (s) ;E °= – 0.44 V
Calculate ΔG° for the net process.
(a) –322 kJmol^–1
(b) –161 kJmol^–1
(c) –152 kJmol^–1
(d) –76 kJmol^–1               

Question. The cell, Zn| Zn (1M) | | Cu (1M)| Cu 2+ 2+
(E °cell = 1.10 V), was allowed to be completely discharged at 298 K. The relative concentration of Zn²⁺ to Cu²⁺ {[Zn²⁺ / Cu²⁺] 2+   [Zn ] [Cu ] is
(a) antilog (24.08)
(b) 37.2
(c) 10^37.2
(d) 9.65 × 10⁴               

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