JEE Chemistry - MCQ Practice Questions

During the electrolysis of CuSO₄ solution with copper electrodes, which of the following occurs?

If the equilibrium constant K for a reaction at 25°C is 10¹⁰, what is the approximate standard cell potential? (Use F ≈ 96500 C/mol, R = 8.314 J/mol·K)

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:

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?

Two cells with the same emf but different internal resistances are connected. Which cell will deliver more current in an external circuit?

A galvanic cell has E°cell = +1.2 V at 25°C with n = 2. At what concentration ratio [Zn²⁺]/[Ag⁺] will the cell potential equal zero?

In electrochemistry, overpotential is important because:

If a current of 10 A is passed through a solution for 30 minutes, the total charge passed (in Faradays) is approximately:

According to the latest JEE chemistry pattern (2024-25), the conductivity of a strong electrolyte solution depends primarily on:

In an electrochemical cell at 25°C, if E°cell = +0.30 V and the cell quotient Q = 10, the cell potential using Nernst equation (n=2) is approximately:

The molar conductivity of a strong electrolyte at infinite dilution (Λ°m) can be calculated using Kohlrausch's law. For NaCl, if Λ°m(HCl) = 426, Λ°m(NaOH) = 248, and Λ°m(KCl) = 150, then Λ°m(NaCl) is:

For a reaction with mechanism: A ⇌ B (fast equilibrium), B + C → D (slow), the rate law is:

The rate constant for a reaction increases 4 times when temperature increases from 27°C to 47°C. What is the activation energy? (R = 8.314 J mol⁻¹ K⁻¹)

In a reaction, the rate increases by a factor of 8 when [A] doubles and by a factor of 2 when [B] doubles. What is the overall order of the reaction?