JEE Chemistry - MCQ Practice Questions

The molar conductivity of an electrolyte increases upon dilution because:

During the electrolysis of molten NaCl, the cathode product is:

Which of the following solutions has the highest conductivity?

The equivalent conductivity of a strong electrolyte at infinite dilution (Λ∞) for HCl is approximately:

In a concentration cell, the EMF depends on:

Calculate the number of Faradays required to deposit 3.2 g of Cu (atomic mass 64) from CuSO₄ solution:

In the electrolysis of dilute H₂SO₄ with inert electrodes, the cathode reaction is:

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?

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

The molar conductivity of a solution increases with dilution because:

For the cell reaction: Zn + Cu²⁺ → Zn²⁺ + Cu, if E°(Zn²⁺/Zn) = -0.76 V and E°(Cu²⁺/Cu) = +0.34 V, the standard cell potential is: