JEE Chemistry - MCQ Practice Questions

What is the SI unit of electrical conductivity?

In a galvanic cell, which electrode acts as the negative terminal?

What does Faraday's first law of electrolysis state?

The Nernst equation is used to calculate:

Which of the following is a primary cell (non-rechargeable)?

In electroplating, the object to be plated is connected to which terminal?

What is the relationship between ΔG° and E°cell at 25°C?

A cell has E°cell = +0.34 V. Which statement is correct?

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:

The standard reduction potential for Zn²⁺/Zn is -0.76 V and for Cu²⁺/Cu is +0.34 V. For the cell Zn-Cu, E°cell is:

An electrochemical cell requires 193,700 C of charge to deposit 19.6 g of a metal X. The valency of metal X is:

At 25°C, for a cell reaction: Zn(s) + 2Ag⁺(aq) → Zn²⁺(aq) + 2Ag(s), if [Zn²⁺] = 1 M and [Ag⁺] = 0.1 M, and E°cell = 1.56 V, the Ecell is approximately:

The conductivity of a solution containing 0.1 M NaCl is 1.29 S·m⁻¹. The molar conductivity is:

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

In a galvanic cell, oxidation occurs at which electrode?