JEE Chemistry - MCQ Practice Questions

The Faraday constant (F) is approximately equal to:

Which statement is correct regarding electrode potentials?

For a spontaneous electrochemical cell, the cell potential (E°cell) should be:

The Nernst equation relates cell potential to which of the following?

In the electrolysis of aqueous KCl solution with inert electrodes, which gas is produced at the cathode?

The cell potential at 25°C for the reaction: Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s) is 0.46 V. Calculate ΔG°:

Which metal cannot be obtained by electrolysis of its aqueous salt solution?

In a concentration cell with two zinc electrodes in different concentrations of Zn²⁺, which statement is true?

The molar conductivity of a solution decreases with dilution for:

What is the purpose of a salt bridge in an electrochemical cell?

For the electrode reaction: MnO₄⁻ + 8H⁺ + 5e⁻ → Mn²⁺ + 4H₂O, the number of electrons transferred in the redox reaction is:

Using the data: E°(Cu²⁺/Cu) = +0.34 V, E°(Zn²⁺/Zn) = -0.76 V, what is E°cell for the Daniell cell?

In electroplating of iron with copper, which electrode should be made of copper?

At 25°C, the relationship between ΔG° and K (equilibrium constant) is given by:

For the cell: Pt | H₂(1 atm) | H⁺(0.1 M) || Ag⁺(0.1 M) | Ag, calculate E at 25°C if E°cell = 0.80 V and log(0.1) = -1:

The conductivity of a solution is 2.0 × 10⁻⁴ S/cm and the cell constant is 1.0 cm⁻¹. What is the molar conductivity of 0.01 M solution?

In the galvanic cell using Pb-PbSO₄ electrode and Hg-Hg₂Cl₂ electrode (calomel), which is the cathode if E°(Hg₂Cl₂/Hg) = 0.27 V and E°(PbSO₄/Pb) = -0.36 V?

What mass of Cu is deposited when 2 Faradays of charge pass through a CuSO₄ solution? (Atomic mass of Cu = 64)

In a galvanic cell, the electrode where oxidation occurs is called:

The standard cell potential (E°cell) for a reaction is -0.45 V at 25°C. What can be concluded about the reaction?