CBSE Class 12 Chemistry HOTs Electrochemistry

Please refer to CBSE Class 12 Chemistry HOTs Electrochemistry. Download HOTS questions and answers for Class 12 Chemistry. Read CBSE Class 12 Chemistry HOTs for Unit 3 Electrochemistry below and download in pdf. High Order Thinking Skills questions come in exams for Chemistry in Class 12 and if prepared properly can help you to score more marks. You can refer to more chapter wise Class 12 Chemistry HOTS Questions with solutions and also get latest topic wise important study material as per NCERT book for Class 12 Chemistry and all other subjects for free on Studiestoday designed as per latest CBSE, NCERT and KVS syllabus and pattern for Class 12

Unit 3 Electrochemistry Class 12 Chemistry HOTS

Class 12 Chemistry students should refer to the following high order thinking skills questions with answers for Unit 3 Electrochemistry in Class 12. These HOTS questions with answers for Class 12 Chemistry will come in exams and help you to score good marks

HOTS Questions Unit 3 Electrochemistry Class 12 Chemistry with Answers

Question. Saturated solution of KNO3 is used to make ‘salt-bridge’ because:
a. Velocity of K+ is greater than that of NO3−
b. Velocity of NO3− is greater than that of K+
c. Velocities of both K+ and NO3− are nearly the same
d. KNO3 is highly soluble in water
Answer : C

Question. Beryllium is placed above magnesium in the second group. 
Beryllium dust, therefore when added to MgCl2 solution will
a. Have no effect
b. Precipitate Mg metal
c. Precipitate MgO
d. Lead to dissolution of be metal
Answer : A

Question. Which of the following is a highly corrosive salt?
a. FeCl2
b. PbCl2
c. Hg2Cl2
d. HgCl2
Answer : D

Question. Some statements are given below. The correct statements are:
a. The electrolysis of aqueous NaCl produces hydrogen gas at the cathode and chlorine gas at the anode
b. The electrolysis of a dilute solution of sodium fluoride produces oxygen gas at the anode and hydrogen gas at the cathode
c. The electrolysis of concentrated sulphuric acid produces SO2 gas at the anode and O2 gas at the cathode
d. After the electrolysis of aqueous sodium sulphate, the solution becomes acidic
Answer : A, B

Question. A cell constructed by coupling a standard copper electrode and a standard magnesium electrode has emf of 2.7 volts. If the standard reduction potential of copper electrode is + 0.34 volt that of magnesium electrode is:
a. + 3.04 volts
b. – 3.04 volts
c. + 2.36 volts
d. – 2.36 volts
Answer : D

Question. The position of some metals in the electrochemical series in decreasing electropositive character is given as Mg > Al > Zn > Cu > Ag.
What will happen, if a copper spoon is used to stir a solution of aluminium nitrate?
a. The spoon will get coated with Al
b. An alloy of Cu and Al is formed
c. The solution becomes blue
d. There is no reaction
Answer : D

Question. Which of the following statement is true for an electrochemical cell?
a. H2 is cathode and Cu is anode
b. H2 is anode and Cu is cathode
c. Reduction occurs at H2 electrode
d. Oxidation occurs at Cu electrode
Answer : B

Question. Corrosion of iron is essentially an electrochemical phenomenon where the cell reactions are?
a. Fe is oxidised to Fe2+ and dissolved oxygen in water is reduced to nOH
b. Fe is oxidised to Fe3+ and H2O is reduced to O22−
c. s is oxidised to Fe2+ and H2O is reduced to O−2
d. Fe is oxidised to Fe2+ and H2O is reduced to O2
Answer : A

Question. The emf of the following cell is 0.22 V.
Ag(s)AgCl(s) | KCl(1M) | H+ (1M) | H2 (g) (1 atm); Pt(s) 
Which of the following will decreases the EMF of cell?
a. Increasing pressure of H2(g) from 1 atm to 2 atm
b. Increasing Cl–concentration in anodic compartment
c. Increasing H+ concentration in cathodic compartment
d. Increasing KCl concentration in anodic compartment
Answer : A, D

Question. Two half cells have potential –0.76 V and –0.13 V respectively. A galvanic cell is made from these two half cells. Which of the following statements is correct?
a. Electrode of half-cell potential –0.76 V serves as cathode
b. Electrode of half-cell potential – 0.76 V serves as anode
c. Electrode of half-cell potential –0.13 V serves as cathode
d. Electrode of half-cell potential –0.76 V serves as positive electrode and 0.13 V as negative electrode
Answer : B, C

Question. During the purification of copper by electrolysis:
a. The anode used is made of copper ore
b. Pure copper is deposited on the cathode
c. The impurities such as Ag, Au are present in solutions as ions
d. Concentrations of CuSO4, solution remains constant during dissolution of Cu
Answer : A, B, D

Question. When a galvanic cell starts, working with the passage of time
a. Spontaneity of the cell reaction decreases, Ecell decreases
b. Reaction quotient Q decreases Ecellincreases
c. Reaction quotient Q increases Ecell increases
d. At equilibrium Q = Kc and Ecell = 0
Answer : A, D

Question. Which of the following statement(s) is/are correct?
a. F2 is the strongest oxidizing agent
b. Li is the strongest reducing agent
c. Li+ is the weakest oxidizing agent
d. F2 is highest reduction potential
Answer : B, C

Question. If 96500 coulomb electricity is passed through CuSO4 solution, it will liberate
(a) 63.5 gm of Cu
(b) 31.76 gm of Cu
(c) 96500 gm of Cu
(d) 100 gm of Cu
Answer. B

Question. Fused NaCl on electrolysis gives ………….. on cathode.
(a) Chlroine
(b) Sodium
(c) Sodium amalgam
(d) Hydrogen
Answer. B

Question. Molar conductivity of 0.15 M solution of KCl at 298 K, if its conductivity of 0.0152 S cm-1 will be
(a) 124 Ω-1 cm² mol-1
(b) 204 Ω-1 cm² mol-1
(c) 101 Ω-1 cm² mol-1
(d) 300 Ω-1 cm² mol-1
Answer. C

Question. The molar conductivity is maximum for the solution of concentration
(a) 0.004 M
(b) 0.002 M
(c)0.005 M
(d) 0.001 M
Answer. D

Question. How long would it take to deposit 50 g of Al from an electrolytic cell containing Al2O3 using a current of 105 amperes?
(a) 1.54 h
(b) 1.42 h
(c) 1.32 h
(d) 2.15 h
Answer. B

Question. How many coulombs of electricity is required to reduce 1 mole of Cr2O72- in acidic medium?
(a) 4 × 96500 C
(b) 6 × 96500 C
(c) 2 × 96500 C
(d) 1 × 96500 C
Answer. B

Question. When heating one end of a metal plate, the other end gets hot because of
(a) the resistance of the metal
(b) mobility of atoms in the metal
(c) energised electrons moving to the other end
(d) minor perturbation in the energy of atoms.
Answer. C

Question. The equivalent conductance of Ba2+ and Cl– are respectively 127 and 76 ohm-1 cm-1 eq-1 at infinite dilution. The equivalent conductance of BaCl2 at infinite dilution will be
(a) 139.5
(b) 203
(c) 279
(d) 101.5
Answer. A

Question. Standard solution of KNO3 is used to make a salt bridge because
(a) Velocity of K+ is greater than that of NO−3.
(b) Velocity of NO−3 is greater than that of K+.
(c) Velocity of both K+ and NO−3 are nearly same
(d) KNO3 is highly soluble in water.
Answer. C

Question. The amount of electricity required to deposit 1 mol of aluminium from a solution of AlCl3 will be
(a) 0.33 F
(b) 1 F
(c) 3 F
(d) 1 ampere
Answer. C

Question. Which of the following is supplied to the cathode of a fuel cell?
(a) Hydrogen
(b) Nitrogen
(c) Oxygen
(d) Chlorine
Answer. C


ASSERTION REASON TYPE OF QUESTIONS
The question given below consist of an assertion and a reason use the following key to choose appropriate answer
a) Both assertion and reason are correct and reason is the correct explanation of the assertion
b) Both assertion and reason are correct and reason is not the correct explanation of the assertion
c) Assertion is correct but reason is incorrect
d) Assertion is wrong Reason is correct.

Question. Assertion: The electrode potential of SHE is zero
Reason: In SHE HCl 1M and H2 gas at one bar pressure is taken
Answer. B

Question. Assertion: H+ ion cannot oxidize copper
Reason: Reduction potential of Cu2+ / Cu is greater than H+/H
Answer. A

Question. Assertion: The reduction potential of F-/F is highest among all electrodes
Reason: Fluorine is the strongest oxidising agent
Answer. B

Question. Assertion: Electronic conduction decreases with temperature
Reason: The flow of electrons hindered on increasing the temperature
Answer. A

Question. Assertion: conductivity decreases with increasing dilution
Reason: No of ions increases per unit volume increases with dilution.
Answer. C

Question. Assertion: Electrolytic conduction increases with temperature
Reason: On increasing the temperature mobility of ion increases
Answer. A

Question. Assertion: Molar conductivity of electrolytes decreases with dilution
Reason: For weak electrolytes degree of dissociation increases with dilution.
Answer. D

Question. Assertion: It is difficult to measure the conductivity of ionic solutions
Reason: Electrolytes conduct electricity and undergoes chemical change.
Answer. A

Question. Assertion: Molar conductivity of strong electrolytes increases with dilution
Reason: On dilution inter ionic interaction increases.
Answer. C

Question. Assertion: Molar conductivity of acetic acid increases sharply with dilution
Reason: Degree of dissociation of acetic acid decreases with dilution
Answer. C

Question. Assertion:An external potential of 1.1V is passed through Danielcell, no current flow through it.
Reason: Standard emf of galvanic cell is 1.1 volt.
Answer. B

Question. Assertion: Out of Li and K Potassium is the strongest reducing agent
Reason: Reduction potential of K is greater than that of Li
Answer. D

Question. Assertion: Electrolytic conduction of electrolytes depends on size of ions
Reason: Larger the size of ion lesser will be the mobility of ions.
Answer. A

Question. Assertion: Limiting molar conductivity of weak electrolytes can be obtained graphically
Reason: Limiting molar conductivity of weak electrolytes increases with dilution
Answer. B

Question. Assertion: Electrolysis of aqueous NaCl produces Oxygen at the anode
Reason: Oxidation potential of Oxygen is lower than chlorine.
Answer. D


SHORT ANSWER TYPE QUESTIONS

Question. Define the following terms : (i) Molar conductivity (Λm) (ii) Secondary batteries
Answer. Molar conductivity of a solution at a given concentration is the conductance of the volume ‘V’ of a solution containing one mole of electrolyte kept between two electrodes with area of cross section ‘A’ and distance of unit length. It is represented by Λm. Unit of Λm is S cm2 mol-1
Λm = 𝑘c x 1000/Molarity Secondary batteries are those batteries which can be recharged by passing an electric current through them and can be used again and again are called secondary batteries.

Question. Calculate the time to deposit 1.27 g of copper at cathode when a current of 2A was passed through the solution of CuSO4. (Molar mass of Cu = 63.5 g mol-1,1 F = 96500 C mol-1)
Answer. CuSO4 → Cu+ + SO42-
Cu2+ + 2e– → Cu
63.5 gram of copper is deposited = 2 × 96500 C
1.27 gram of Cu is deposited =( 2×96500/63.5) × 1.27
= 3860
Q = I × t
3860 = 2 x t
t = 3860/2 = 1930 seconds

Question. Write the name of the cell which is generally used in transistors. Write the reactions taking place at the anode and the cathode of this cell.
Answer. Leclanche cell is used in transistors.
Reaction at Anode: Zn(s) → Zn2+ + 2e–
At Cathode: MnO2 + NH4+ + e– → MnO(OH) + NH3


1. Read the given passage and answer the questions 1 to 5 that follow:
"Car battery is the most important type of secondary cell having a lead anode and a grid of Lead packed with PbO2 as cathode. It is also called lead storage battery. It contains 40% solution of sulphuric acid (Density = 1.294 gmL-1) as electrolyte. The battery holds 3.5 L of the acid. During the discharge of the battery, the density of H2SO4 falls to 1.139 gmL-1 (20% H2SO4 by mass)"

Question. Write the reaction taking place at the cathode when the battery is in use.
Answer. Cathode reaction is
PbO₂ + SO2 + 4H+ + 2e- → 2PbSO4 + 2H₂O

Question. How much electricity in terms of Faraday is required to carry out the reduction of one mole of PbO2
Answer. 2F

Question. What is the molarity of sulphuric acid before discharge?
Answer. Molarity = (% ×10 ×d) ÷ (Molarity of H2SO4) = (40 x 10 x 1.294) ÷ 98 = 5.28 mol L-1

Question. Why is lead storage battery considered a secondary cell?
Answer. It can be recharged again and again.

Question. Write the products of electrolysis when dilute sulphuric acid is electrolysed using platinum electrodes.
Answer. H2 at cathode and O2 at anode.

Question. A steady current of 2 amperes was passed through two electrolytic cells X and Y connected in series containing electrolytes FeSO4 and ZnSO4 until 2.8g of Fe deposited at the cathode of cell X. How long did the current flow ? Calculate the mass of Zn deposited at the cathode of cell Y. (Molar mass : Fe = 56 g mol–1 Zn = 65.3 g mol–1, 1F = 96500 C mol–1)
Answer. (a) 𝑚 = 𝑧 𝐼 𝑡
2.8 g = (56 ×2 ×𝑡)/2 ×96500
t= 4825 s 0r 80.417 min
𝑚1 / 𝑚2 = 𝐸1 /𝐸2
2.8/ 𝑚𝑍𝑛 = (56 / 2) X( 2 / 65.3)
mZn = 3.265 g 

Question. (a) Out of the following pairs, predict with reason which pair will allow greater conduction of electricity :
(i) Silver wire at 30oC or silver wire at 60oC.
(ii) 0·1M CH3COOH solution or 1M CH3COOH solution.
(iii) KCl solution at 200C or KCl solution at 50oC.
(b)Give two points of differences between electrochemical and electrolytic cells. (3+2)
Answer. (a) (i) Silver wire at 300C because as temperature decreases, resistance decreases so conduction increases.
(ii) 0.1 M CH3COOH, because on dilution degree of ionization increases hence conduction increases.
(iii) KCl solution at 500C, because at high temperature mobility of ions increases and hence conductance increases
(b) Electrochemical cell
(1) Anode -ve Cathode +ve
(2) Convert chemical Energy to electrical energy Electrolytic cell
(1) Anode +ve ,Cathode -ve
(2) Convert electrical Energy to chemical energy (or any other correct differences)

Question. a) Write the Nernst equation for the following cell reaction: Zn(s)+Cu2+(aq) ➔ Zn2+(aq)+Cu(s)
b) How will the E cell be affected when concentration of
(i)Cu 2+ ions is increased and (ii) Zn 2+ ions is increased ?
Answer. a) Zn(s)|Zn2+(aq)|| Cu2+(aq)|Cu(s)
b) (i) E(cell) increases (ii) E(cell) decreases

Question. (a) The standard Gibbs energy (ΔrG0 ) for the following cell reaction is -300 kJ mol-1:
Zn(s) + 2Ag + (aq) ➔ Zn 2+ (aq) + 2Ag(s) 
Calculate E0 cell for the reaction. (Given: lF = 96500 moI-1 )
Answer. ΔrG0 =-nFE0(cell)
-300x1000j/mol=-2x96500xE0(cell)
E0(cell)=300000/2x96500=1.55v

Question. Calculat λ0m for MgCl2 if λ0 values for Mg2+ ion and Cl - ion are 106 S cm2mol-1 and 76.3 S cm2mol--1respectively.
Answer. Λ0m MgCl2 = λ0Mg2++ λ02Cl-
= 106 Scm2mol—1+76.3x2 Scm2mol—1
= 258.6 Scm2mol

 
1 - MARK QUESTIONS
 
1.1F of electricity deposits 1 mole of Na from the molten salt, but 1/3 mol of Al from an aluminium salt. Why ? 
2. What is the role of ZnCl2 in the dry cell ? 
3. Why blocks of Mg are often strapped to the steel hulls of ocean going ships ? 
4. Which of the Li+ and Na+ have the greater mobility in aq solution ? Why ? 
5. Corrosion of motor cars is of greater problem in winter when salts are spread on roads to melt ice and snow. Why ? 
 
 
2 - MARKS QUESTIONS
 
6. Which will have greater molar conductivity and why ? 
a. 1 mole KCl dissolved in 200 cc of the solution
b. 1 mole KCl dissolved in 500 cc of the solution. 
7. Why is Li best reducing agent where as Fluorine is best oxidizing agent ? 
8. Equilibrium constant is related to Eθcell but not to Ecell . Explain.
9. Why sodium metal is not obtained at cathode when aq NaCl is electrolysed with Pt electrodes but obtained when moleten NaCl is electrolysed ? 
10. Zn rod weighing 25 g was kept in 100 mL of 1M copper sulphate solution. After certain time interval, the molarity of Cu2+ was found to be 0.8 M. What is the molarity of SO42- in the resulting solution and what should be the mass of Zn rod after cleaning and drying ?
 
 
3 - MARKS QUESTIONS
 
11. A cell contains two hydrogen electrodes. The negative electrode is in contact with a solution of 10-6 M H+ ions. The emf of the cell is 0.118 V at 298 K. Calculate the concentration of the H+ ions at the positive electrode. 
12. Crude copper containing Fe and Ag as contaminations was subjected to electro refining by using a current of 175 A for 6.434 min. The mass of anode was found to decrease by 22.260 g, while that of cathode was increased by 22.011 g. Estimate the % of copper, iron and silver in crude copper.
13. Zinc electrode is constituted at 298 K by placing Zn rod in 0.1 M aq solution of zinc sulphate which is 95 % dissociated at this concentration. What will be the electrode potential of the electrode given that EΘZn2+/Zn =-0.76V.
14. At what pH will hydrogen electrode at 298 K show an electrode potential of -0.118 V, when Hydrogen gas is bubbled at 1 atm pressure ?
15. Electrolysis of the solution of MnSO4 in aq sulphuric acid is a method for the preparation of MnO2 as per the chemical reaction
Mn2+ + 2H2O → MnO2 + 2H+ + H2
Passing a current of 27 A for 24 Hrs gives 1 kg of MnO2. What is the current efficiency ? What are the reactions occurring at anode and cathode ?

 

2 Marks Questions

1 How many faraday of charge is required for conversion of C6H5NO2 into C6H5NH2? 
2 Explain why Zn dissolves in dil. HCl to liberate H2(g) but from conc. H2SO4, the gas evolved is SO2.
3 Cu does not dissolve in HCl but dissolves in nitric acid. Explain why?
4 Fluorine has a low electron gain enthalpy compared to chlorine, yet it is a more powerful oxidant. Explain why?
5 If Zn2+/Zn electrode is diluted 100 times, then what will be the change in emf?
6 You are aquainted with the construction and working of a lead-storage battery. Give the plausible reasons for these facts:
1. There is only a single compartment unlike other electrochemical cells.
2. Replacement of water is necessary for maintenance.
7 For what concentration of Ag+(aq.), will the emf of given cell be zero at \ 25oC , if the concentration of Cu(s) | Cu2+(0.1M) || Ag+(aq.) | Ag(s)? Given , E0 Ag+/Ag=0.80V; E0 Cu2+/Cu=0.34V.
 8 In a small town along the costal area, it is observed that iron objects rust easily. Being an industrial town, it also faces air pollution problem. Identify any 4 factors which are contributing to rusting phenomenon.
9 Iodine(I2) and Bromine(Br2) are added to a solution containing iodide(I-) and bromide ions(Br-). What reaction would occur if the concentration of each species is 1M? The electrode potentials are E0 I2/I-=0.54V and E0 Br2/Br-=1.08V

 
3 Marks Questions
 
10 In an industrial plant, aluminium is produced by elecrolysis of alumina dissolved in cryolite. This takes a current of 20000A. If the current efficiency is 90%, how much Al will be produced per day?
11 In an experiment 0.04 F was passed through 400 mL of 1M soln. of NaCl. What would be pH of the soln. after elecrolysis.
12 Estimate the minimum P.D. needed to reduce Al2O3 at 5000 C. The free energy change for the decomposition reaction is 960 kJ.
2/3 Al2O3 4/3 Al + O2;  Δ=960kJ
13. A cell with N/50 KCl soln. offered a resistance of 550 ohms at 298 K. The specific conductance of N/50 KCl at 298 K is 0.002768 ohm-1cm-1. When the cell is filled with N/10 ZnSO4 soln, it offered a resistance of 72.18 ohms at 298 K. Find the cell constant and molar conductance of ZnSO4 soln. at 298K.
14. Which of the following has larger molar conductance:
a. 0.08 M soln. having conductivity equal to 2 × 10-2 ohm-1cm-1.
b. 0.10 M soln. having resistivity equal to 5.8 ohm cm.
15. The Ksp of AgCl at 298 K is 1 × 10-10. Calculate electrode potential of Ag electrode immersed in 1 M KCl soln.
[Given: E0 Ag+/Ag = 0.799 V ]
16. Tarnished siver contains Ag2S. Can this tarnish be removed by immersing the tarnished silverware in an Al pan containing an inert electrolyte soln. such as NaCl?
Given that standard electrode potentials for half reactions are:
Ag2S(s) + 2e- 2Ag(s) + S2-(aq.) is -0.71 V
Al3+(aq.) + 3e- Al(s) is -1.66 V.
17 Observe the diagram carefully and answer the questions below:
An external opposite potential is applied such that it exceeds the cell potential.
a. Is this an electrochemical cell or electrolytic cell?
b. Which substance gets dissolved?
c. Which substance gets deposited and where?
d. Write half cell reactions.
e. Is the needle in the voltmeter correctly marked?
18 2 beakers A and B contain 1 M ZnSO4 solution. To A , Strip of Mg is dipped, while in B, A zinc rod is put. If both are connected to a standard hydrogen electrode, which cell would show a deflection? Explain with suitable reason.
19 The standard electrode potentials of different electrodes are given as
E0 Co3+ /Co2+ = 1.81 V,           E0Al3+/Al = -1.66 V,           E0Fe2+/Fe = -0.44 V,        E0 Br2/Br- = 1.01 V
a. Identify all the possible combination for construction of a feasible electrochemical cell?
b. Write their electrochemical cell representation.
c. Calculate the emf in each case.
20 a. During electrolysis of NaOH, Cl2 and H2 while for molten NaCl only Na metal and Cl2 gas are obtained. Explain these observations with suitable eqn.
b. Electrolysis of conc. and dil. sulphuric acid are different. Explain with eqn.
21 An Aq. solution of AuCl3 was electrolysed with a current of 0.5A until 1.20g of Au had been deposited on the cathode. At another electrode in series with this, the only reaction was evolution of O2. Find—
1. The no. of moles
2. The volume at NTP
3. The mass of O2 liberated
4. the no. of coulombs passed through the solution and
5. the duration of electrolysis
 
Unit 01 The Solid State
CBSE Class 12 Chemistry HOTs The Solid State
Unit 02 Solutions
CBSE Class 12 Chemistry HOTs Solutions
Unit 03 Electrochemistry
CBSE Class 12 Chemistry HOTs Electrochemistry
Unit 04 Chemical Kinetics
CBSE Class 12 Chemistry HOTs Chemical Kinetics
Unit 05 Surface Chemistry
CBSE Class 12 Chemistry HOTs Surface Chemistry
Unit 06 General Principles and Processes of Isolation of Elements
CBSE Class 12 Chemistry HOTs General Principles And Processes Of Isolation Of Elements
CBSE Class 12 Chemistry HOTs Isolation of Elements
Unit 07 The p-Block Elements
CBSE Class 12 Chemistry HOTs p Block Elements
Unit 08 The d- and f-Block Elements
CBSE Class 12 Chemistry HOTs d and f block Elements
Unit 09 Coordination Compounds
CBSE Class 12 Chemistry HOTs Coordination Compounds
Unit 10 Haloalkanes and Haloarenes
CBSE Class 12 Chemistry HOTs Haloalkanes And Haloarenes
Unit 11 Alcohols, Phenols and Ethers
CBSE Class 12 Chemistry HOTs Alcohols Phenols And Ethers
Unit 12 Aldehydes, Ketones and Carboxylic Acids
CBSE Class 12 Chemistry HOTs Aldehyde Ketones And Carboxylic Acids
Unit 13 Amines
CBSE Class 12 Chemistry HOTs Animes
Unit 14 Biomolecules
CBSE Class 12 Chemistry HOTs Biomolecules
Unit 15 Polymers
CBSE Class 12 Chemistry HOTs Polymers
Unit 16 Chemistry in Everyday Life
CBSE Class 12 Chemistry HOTs Chemistry in Everyday Life
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HOTS for Unit 3 Electrochemistry Chemistry Class 12

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