75 free MCQs on Electrochemistry, each with its own worked answer and explanation. Explore the link between chemical reactions and electricity. Covers galvanic cells, electrolysis, standard electrode potentials, the Nernst equation, and real-world applications like batteries and corrosion.
Take the timed Electrochemistry chapterwise test →75 practice questions on Electrochemistry, sorted Easy → Hard. Try each one first, then open its answer page for the worked explanation. Want the full theory first? Read the Electrochemistry notes.
In a Daniell cell, electrons flow externally from the zinc anode (oxidation) through the voltmeter to the copper cathode (reduction), while the salt bridge completes the circuit.
Q1.
In the lead storage battery, the anode (negative electrode) is made of:
Q2.
The SI unit of molar conductivity is:
Q3.
Which of the following is a primary cell?
Q4.
In a hydrogen-oxygen fuel cell, the product formed is:
Q5.
With an increase in temperature, the conductivity of an electrolytic solution generally:
Q6.
Electrolysis uses electricity to:
Q7.
In an electrolytic cell, reduction occurs at the:
Q8.
In a galvanic cell, the anode is the:
Q10.
The standard hydrogen electrode is assigned a potential of:
Q11.
Which process always occurs at the anode?
Q12.
One Faraday (F) is the charge carried by:
Q13.
In the Daniell cell, which metal acts as the anode?
Q14.
The conductivity of a metallic conductor with increasing temperature:
Q15.
Faraday's first law of electrolysis states that mass deposited is proportional to:
Q16.
A device that converts chemical energy into electrical energy is a:
Q17.
In a galvanic cell, oxidation takes place at the:
Q18.
In any electrochemical cell, reduction occurs at the:
Q19.
The main function of a salt bridge is to:
Q20.
The SI unit of electric charge is the:
Q21.
One faraday of electric charge is approximately:
Q22.
The standard reduction potential of the standard hydrogen electrode is taken as:
Q23.
The rate of flow of electric charge (current) is measured in:
Q24.
Electrolysis is the decomposition of a compound brought about by passing:
Q25.
In the electrochemical series, a species that is more easily reduced has a:
Q26.
Electrolysis of aqueous sodium chloride (brine) produces at the cathode:
Q27.
The quantity of electricity required to liberate 1 mole of H<sub>2</sub> gas by the electrolysis of water is:
Q28.
The charge required to deposit 0.5 mol of copper from Cu<sup>2+</sup> solution is (F = 96500 C):
Q29.
A current of 5 A deposits 0.635 g of copper (Cu = 63.5, F = 96500). The time of electrolysis is:
Q30.
Given E°(Cu<sup>2+</sup>/Cu) = +0.34 V and E°(Ag<sup>+</sup>/Ag) = +0.80 V, the standard EMF of the cell Cu | Cu<sup>2+</sup> || Ag<sup>+</sup> | Ag is:
Q31.
The standard EMF of the Daniell cell (Zn-Cu) is approximately:
Q32.
The relationship between ΔG° and E°cell is:
Q33.
During electrolysis of dilute H₂SO₄, the gas at the cathode is:
Q34.
Kohlrausch's law states that at infinite dilution, molar conductance equals:
Q35.
The Nernst equation is used to calculate:
Q36.
Faraday's second law: for the same quantity of charge, masses deposited are proportional to:
Q37.
Molar conductance of an electrolyte solution increases on dilution because:
Q38.
Which device requires an external source of EMF to operate?
Q39.
Why does the conductivity of a strong electrolyte solution decrease as its concentration increases, even though molar conductivity is being measured?
Q40.
In a galvanic cell such as the Daniell cell, electrons flow through the external circuit from the:
Q41.
The standard EMF of a cell is E°cell = E°cathode −:
Q42.
By Faraday’s first law of electrolysis, the mass of a substance deposited is proportional to the:
Q43.
For a spontaneous cell reaction, the standard cell potential E°cell is:
Q44.
The relationship between standard free energy and cell potential is ΔG° =:
Q45.
The conductivity (specific conductance) of an electrolyte solution, on dilution:
Q46.
The molar conductivity of an electrolyte solution, on dilution:
Q47.
Kohlrausch’s law expresses the limiting molar conductivity as the sum of contributions from the individual:
Q48.
During the electrolysis of molten sodium chloride, sodium metal is deposited at the:
Q49.
The number of electrons involved in the reduction Cu²⁺ + 2e⁻ → Cu is:
Q50.
A secondary cell differs from a primary cell in that it can be:
Q51.
During the electrolysis of molten calcium chloride, the mass of calcium deposited by 1 F of charge is (Ca = 40):
Q52.
On passing 0.1 F of charge through molten AlCl<sub>3</sub>, the mass of aluminium deposited is (Al = 27):
Q53.
For a cell with E°<sub>cell</sub> = 0.295 V and n = 2 at 298 K, the value of log K is:
Q54.
The mass of oxygen gas liberated at the anode when 4 F of charge passes through acidified water is (O = 16):
Q55.
Given lambda° values (S cm<sup>2</sup> mol<sup>-1</sup>): HCl = 426, CH<sub>3</sub>COONa = 91, NaCl = 126. The lambda° for acetic acid is:
Q56.
For Zn|Zn²⁺(0.1M)||Cu²⁺(0.01M)|Cu with E°cell = 1.10 V at 298 K, the cell EMF is:
Q57.
Mass of silver deposited when 2 A passes for 1930 s (Ag = 108, F = 96500 C) is:
Q58.
Electrode potential of Cu²⁺/Cu when [Cu²⁺] = 0.01 M at 298 K (E° = +0.34 V) is:
Q59.
Which electrode has the highest standard reduction potential?
Q60.
The Debye-Huckel-Onsager equation for molar conductance vs concentration is:
Q61.
In electrolysis of aqueous CuSO₄ using Pt electrodes, what forms at the anode?
Q62.
For a cell with E = 1.1 V and n = 2, the Gibbs energy change is:
Q63.
In a concentration cell, the EMF is generated because:
Q64.
A current of 0.5 A is passed through molten Al<sub>2</sub>O<sub>3</sub> for 4825 seconds. What mass of aluminium is deposited (Al = 27 g/mol, F = 96500 C)?
Q65.
For the cell reaction Ni(s) + Cu<sup>2+</sup>(aq) -> Ni<sup>2+</sup>(aq) + Cu(s) with E°cell = 0.57 V at 298 K, what is the equilibrium constant K for this reaction (n = 2)?
Q66.
In the Nernst equation E = E° − (0.059/n) log Q at 298 K, n represents the number of:
Q67.
The quantity of charge required to deposit one mole of aluminium from Al³⁺ is:
Q68.
The mass of copper deposited by passing 2 faradays of charge through CuSO₄ solution is (Cu = 63.5):
Q69.
The molar conductivity of an electrolyte at infinite dilution is called its:
Q70.
For a concentration cell, the standard cell potential E°cell is:
Q71.
The equation E°cell = (0.059/n) log Kc allows calculation of the:
Q72.
The electrolyte used in a common lead storage battery is:
Q73.
The cell constant of a conductivity cell is equal to:
Q74.
If the standard cell potential E°cell is positive, the equilibrium constant K of the reaction is:
Q75.
The rusting of iron in moist air is fundamentally a(n):
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