JEE Chemistry - MCQ Practice Questions

When 3 Faradays of charge are passed through a solution of Cu²⁺, how many moles of Cu are deposited?

The relationship between standard Gibbs free energy change (ΔG°) and equilibrium constant (K) at 25°C is best represented by:

In the electroplating of an object with silver, which electrode should be made of silver?

The specific conductance of a solution is 0.02 S/cm and the cell constant is 1.2 cm⁻¹. The molar conductance of 0.1 M solution is:

Which of the following factors does NOT affect the rate of electrodeposition?

For a galvanic cell at 25°C, E°cell = +0.50 V and n = 2. The value of ΔG° is approximately:

The Nernst equation at 25°C for a cell reaction with n electrons transferred is given by: E = E° - (0.059/n) log Q. What does Q represent?

In the electrolysis of CuSO₄ solution with copper electrodes, what happens at the cathode?

The molar conductivity of strong electrolytes follows which relationship with concentration?

A current of 5 A is passed through an electrolytic cell for 1930 seconds. Calculate the number of moles of electrons transferred. (Faraday constant = 96500 C/mol)

The relationship between equivalent conductance (Λ) and molar conductance (Λm) is:

During the electrolysis of aqueous CuSO₄ solution with copper electrodes, which reaction occurs at the cathode?

The Gibbs free energy change for an electrochemical cell reaction is related to cell potential by:

In the electrorefining of copper, impure copper acts as:

In the electrolysis of dilute H₂SO₄ with inert electrodes, if 2 moles of electrons flow, what volume of gases (in liters at STP) will be produced?

The cell potential of a galvanic cell decreases during operation because:

For the reaction: Fe³⁺ + e⁻ → Fe²⁺ (E° = +0.77 V) and Cl₂ + 2e⁻ → 2Cl⁻ (E° = +1.36 V), which is the strongest oxidizing agent?

During the electrolysis of molten NaCl using inert electrodes, if 2.3 g of Na is deposited at the cathode, what volume of Cl₂ gas (at STP) will be released at the anode?

A galvanic cell is constructed using Zn|Zn²⁺ and Cu|Cu²⁺ half-cells. If the concentration of Zn²⁺ is increased from 1 M to 10 M at 25°C, how does this affect the cell potential? (E°cell = 1.1 V)

For a first-order reaction, if the initial concentration is [A]₀ = 0.5 M and after 30 seconds it becomes 0.25 M, what is the rate constant?