Given below are two statements: Statement-I: 1F electricity is required for the oxidation of 1 mole $\mathrm{H}_2 \mathrm{O}$ to $\mathrm{O}_2.$ Statement-II: To get 40 gm Ca from molten $\mathrm{CaCl}_2$ required electricity is 2F.

Both Statement I and Statement II are incorrect

Statement I is correct but Statement II is incorrect

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Electro chemistry practice · Medium

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31 Medium

31 of 145

Application +4 | -1

How much time is required to decompose 18 g water electrolytically into

{H_2}

and

{O_2}

by passing 3A current?

View answer and explanation

Correct option: B

17.87 hours

Option B is correct because the time required to decompose 18g of water electrolytically is calculated using Faraday's laws of electrolysis, resulting in approximately 17.87 hours.

32 Medium

32 of 145

Analyzing +4 | -1

Which of the following statements is wrong ?

View answer and explanation

Correct option: C

\Delta \mathrm{G}^{\circ}=\mathrm{nFE}^{\circ}

for a spontaneous reaction

Option C is wrong because for a spontaneous reaction,

\Delta G^\circ = -nFE^\circ

, not

\Delta G^\circ = nFE^\circ

33 Medium

33 of 145

Understanding +4 | -1

In the concentration cells, the electrical energy is produced due to :

View answer and explanation

Correct option: D

Transfer of a substance from one concentration to other

Option D (Transfer of a substance from one concentration to other) is correct because concentration cells produce electrical energy due to the difference in concentration between the two half-cells.

34 Medium

34 of 145

Remembering +4 | -1

The factor temperature coefficient of e.m.f. is :

View answer and explanation

Correct option: A

{\left( {\partial E/\partial T} \right)_P}

Option A (

{\left( {\partial E/\partial T} \right)_P}

) is correct because the temperature coefficient of emf is defined as the change in emf with respect to temperature at constant pressure.

35 Medium

35 of 145

Understanding +4 | -1

When Cu reacts with

\mathrm{AgN}{\mathrm{O}_3}

solution, the reaction takes place is

View answer and explanation

Correct option: A

Oxidation of Cu

Option A (Oxidation of Cu) is correct because Cu loses electrons to form

Cu^{2+}

ions when it reacts with

AgNO_3

solution.

36 Medium

36 of 145

Understanding +4 | -1

The value of equilibrium constant for a feasible cell reaction is :

View answer and explanation

Correct option: D

> 1

Option D (> 1) is correct because for a feasible (spontaneous) cell reaction, the equilibrium constant must be greater than 1, indicating that the products are favored.

37 Medium

37 of 145

Analyzing +4 | -1

Among the following which is the strongest oxidizing agent?

View answer and explanation

Correct option: A

M{n^{3 + }}

Option A (

Mn^{3+}

) is the strongest oxidizing agent because

Mn^{3+}

has a strong tendency to get reduced to

Mn^{2+}

, thus oxidizing other species.

38 Medium

38 of 145

Analyzing +4 | -1

Assertion: More negative the electrode potential greater is the power to act as oxidising agent.

Reason: As the electrode potential becomes more negative there is greater tendency to undergo oxidation.

View answer and explanation

Correct option: D

Assertion is wrong, but reason is correct statement.

Option D is correct because a more negative electrode potential indicates a greater tendency for reduction, not oxidation, making the assertion wrong, while the reason is correct.

39 Medium

39 of 145

Remembering +4 | -1

An electronic conductor is

View answer and explanation

Correct option: C

Ag

Option C (

Ag

) is the correct answer because silver is a metal and conducts electricity through the movement of electrons.

40 Medium

40 of 145

Remembering +4 | -1

Cathode used in Leclanche cell is

View answer and explanation

Correct option: B

Graphite rod surrounded by

Mn{O_2}

and carbon

Option B (Graphite rod surrounded by

Mn{O_2}

and carbon) is correct because this is the standard cathode composition in a Leclanche cell.

41 Medium

41 of 145

Application +4 | -1

If the standard electrode potential for a cell

A_{\left( {aq} \right)}^{2 + } + 2{B_{\left( s \right)}} \to {A_{\left( s \right)}} + 2B_{\left( {aq} \right)}^ +

is 1.9 V, then the standard Gibbs energy for the reaction is

View answer and explanation

Correct option: C

-3.8 F J/mol

Option C is correct because the standard Gibbs energy is calculated using the formula

\Delta G = -nFE^\circ

, where n=2 and E° = 1.9 V.

42 Medium

42 of 145

Analyzing +4 | -1

Statement I:

96,500 \mathrm{C}

charge is required for the reduction of one mole of silver ions.

Statement II: The amount of electricity (or) charge required for oxidation or reduction depends on the stoichiometry of the electrode reaction.

View answer and explanation

Correct option: B

If both Statement I and Statement II are correct and Statement II is not a correct explanation of Statement I

Option B is correct. Statement I is correct because the reduction of one mole of silver ions (Ag+) requires one Faraday of charge (96,500 C). Statement II is also correct, but it doesn't explain statement I.

43 Medium

43 of 145

Remembering +4 | -1

The equation representing kohlrausch law from the following is (

{V^ + } =

No. of cations,

{V^ - } =

No. of anions)

View answer and explanation

Correct option: B

\lambda _m^\mathrm{o} = {V^ + }\lambda _ + ^\mathrm{o} + {V^ - }\lambda _ - ^\mathrm{o}

Option B is the correct representation of Kohlrausch's law, stating that the limiting molar conductivity of an electrolyte is the sum of the contributions of the individual ions.

44 Medium

44 of 145

Analyzing +4 | -1

The reaction occurring at anode when the electrolysis of an aqueous solution containing

\mathrm{Na}_2 \mathrm{SO}_4

and

\mathrm{CuSO}_4

is done using

\mathrm {Pt}

electrode is

View answer and explanation

Correct option: C

2 \mathrm{H}_2 \mathrm{O} \longrightarrow \mathrm{O}_2+4 \mathrm{H}^{+}+4 \mathrm{e}

Option C (

2 \mathrm{H}_2 \mathrm{O} \longrightarrow \mathrm{O}_2+4 \mathrm{H}^{+}+4 \mathrm{e}

) is correct because in the electrolysis of aqueous Na2SO4 and CuSO4 using Pt electrodes, water is oxidized at the anode to produce oxygen, hydrogen ions, and electrons.

45 Medium

45 of 145

Remembering +4 | -1

The unit of equivalent conductivity is

View answer and explanation

Correct option: D

\mathrm{oh}{\mathrm{m}^{ - 1}}\,\,\mathrm{c}{\mathrm{m}^\mathrm{2}}\,{\mathrm{(g}\,\,\mathrm{equivalent})^{ - 1}}

Option D is the correct unit for equivalent conductivity, representing conductance per gram equivalent per unit area.

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46 Medium

46 of 145

Understanding +4 | -1

Which one of the following nitrates will leave behind A metal on strong heating?

View answer and explanation

Correct option: D

Silver nitrate

Option D (Silver nitrate) is correct because silver is a relatively unreactive metal, and its nitrate decomposes upon heating to leave behind metallic silver.

47 Medium

47 of 145

Remembering +4 | -1

Cell constant of a conductivity cell is usually derived by using a solution of :

View answer and explanation

Correct option: A

\mathrm{KCl}

Option A (

\mathrm{KCl}

) is correct because potassium chloride (KCl) solutions are commonly used to determine the cell constant due to their well-established conductivity values at various concentrations.

48 Medium

48 of 145

Understanding +4 | -1

The product obtained from the electrolytic oxidation of acidified sulphate solutions, is

View answer and explanation

Correct option: B

H{O_3}SOOS{O_3}H

Option D (

H{O_3}SOS{O_3}H

) is correct because the electrolytic oxidation of acidified sulfate solutions results in the formation of peroxydisulfuric acid (

H_2S_2O_8

), which has the structure

H{O_3}SOS{O_3}H

49 Medium

49 of 145

Remembering +4 | -1

Hydrogen peroxide is obtained by electrolysis of

View answer and explanation

Correct option: B

Sulphurie acid

Option B (Sulphuric acid) is correct because hydrogen peroxide can be obtained by the electrolysis of sulphuric acid.

50 Medium

50 of 145

Remembering +4 | -1

The electrolytic bath used in gold plating of copper articles contains :

View answer and explanation

Correct option: D

\mathrm{AuC}{\mathrm{l}_3} + \mathrm{NaCN}

Option D (

\mathrm{AuC}{\mathrm{l}_3} + \mathrm{NaCN}

) is correct because the addition of NaCN helps in forming a complex with gold, facilitating a smoother and more even plating process.

51 Medium

51 of 145

Analyzing +4 | -1

During the electrolysis of an aqueous salt solution, the

\mathrm{pH}

in the space near one of the electrode was increased and the other one was decreased. The salt solution was

View answer and explanation

Correct option: A

{NaCl}

(very dilute)

Option A is correct. In very dilute NaCl solution, electrolysis produces H+ and OH- ions, changing the pH near the electrodes.

52 Medium

52 of 145

Application +4 | -1

The distance between two electrodes of a cell is 2.5 cm and area of each electrode is

5\mathrm{ }c{m^2}

, then the cell constant (

in\mathrm{ }c{m^{ - 1}}

) is

View answer and explanation

Correct option: D

0.5

Option D is correct because the cell constant is the ratio of the distance between the electrodes to the area of the electrode, which is 2.5 cm / 5 cm² = 0.5 cm⁻¹.

53 Medium

53 of 145

Understanding +4 | -1

On electrolysis of dil. sulphuric acid using Platinum (Pt) electrode, the product obtained at anode will be

View answer and explanation

Correct option: B

Oxygen gas

Option B (Oxygen gas) is correct because during the electrolysis of dilute sulfuric acid, water is oxidized at the anode to produce oxygen gas.

54 Medium

54 of 145

Remembering +4 | -1

One of the commonly used electrode is calomel electrode. Under which of the following categories calomel electrode comes?

View answer and explanation

Correct option: A

Metal - Insoluble Salt - Anion electrodes

Option A (Metal - Insoluble Salt - Anion electrodes) is correct because a calomel electrode consists of mercury (metal), mercurous chloride (insoluble salt), and chloride ions (anion).

55 Medium

55 of 145

Understanding +4 | -1

On dilution which decreases

View answer and explanation

Correct option: B

Option K is correct. The question is incomplete and lacks context. Assuming the question is related to conductivity, 'K' likely refers to conductivity which decreases on dilution.

56 Medium

56 of 145

Analyzing +4 | -1

Which of the following option does not correctly represent the correct order of the property indicated against it ?

View answer and explanation

Correct option: C

Mn\mathrm{ } > Cr\mathrm{ } > \mathrm{ }V\mathrm{ }:\,{E^0}\left( {{M^{3 + }}/{M^{2 + }}} \right)

Option C (

Mn\mathrm{ } > Cr\mathrm{ } > \mathrm{ }V\mathrm{ }:\,{E^0}\left( {{{M^{3 + }}/{M^{2 + }}}} \right)

) is the incorrect order because the actual order is Cr > Mn > V for the given reduction potential.

57 Medium

57 of 145

Analyzing +4 | -1

Assertion (A): Copper sulphate solution is stored in zinc pot.

Reason (R): Zinc is more reactive than copper so it displaces copper from copper sulphate solution.

View answer and explanation

Correct option: D

Assertion is incorrect but Reason is correct.

Option D is correct. The assertion is incorrect because copper sulphate cannot be stored in a zinc pot due to a redox reaction. The reason is correct because zinc is more reactive than copper.

58 Medium

58 of 145

Analyzing +4 | -1

Aqueous solution of

AgNO_3

is electrolyzed using inert electrodes. At the end of electrolysis

View answer and explanation

Correct option: B

P^H

of the solution decreases

Option B (

P^H

of the solution decreases) is correct because during the electrolysis of

AgNO_3

H^+

ions are produced at the anode, leading to a decrease in pH.

59 Medium

59 of 145

Remembering +4 | -1

Prevention of corrosion of iron by zinc coating is called

View answer and explanation

Correct option: D

Galvanization

Option D (Galvanization) is correct because it is the process of coating iron with zinc to prevent corrosion.

60 Medium

60 of 145

Analyzing +4 | -1

Given below are two statements:

Statement-I: 1F electricity is required for the oxidation of 1 mole

\mathrm{H}_2 \mathrm{O}

\mathrm{O}_2.

Statement-II: To get 40 gm Ca from molten

\mathrm{CaCl}_2

required electricity is 2F.

View answer and explanation

Correct option: C

Statement I is incorrect but Statement II is correct

Option C is correct. Statement I is incorrect because the oxidation of 1 mole of H2O to O2 requires 4F of electricity. Statement II is correct because to get 40g Ca from molten CaCl2 requires 2F.

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