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NEET UG Unit 9B1: Electrochemical Cells and Standard Potentials — practice questions

Explore 23 free Unit 9B1: Electrochemical Cells and Standard Potentials questions in NEET UG Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Unit 9B1: Electrochemical Cells and Standard Potentials questions and exercises with answers

Showing questions 1–23 of 23.

In a galvanic cell, the oxidation half-reaction takes place at the:Read the answer and worked solution →In the standard Daniell cell (Zn|Zn²⁺ || Cu²⁺|Cu) at unit concentrations, the cell EMF is:Read the answer and worked solution →The standard hydrogen electrode (SHE) is assigned a standard electrode potential of:Read the answer and worked solution →The Nernst equation for the cell reaction aA + bB → cC + dD at 298 K is:Read the answer and worked solution →For the cell Zn | Zn²⁺ || Cu²⁺ | Cu at 298 K, the Nernst equation expresses E_cell as:Read the answer and worked solution →For the cell Cu(s) + 2Ag⁺ → Cu²⁺ + 2Ag, E°_cell = +0.46 V at 298 K. The equilibrium constant K_c is approximately:Read the answer and worked solution →The relation between cell EMF and Gibbs free-energy change is:Read the answer and worked solution →The SI unit of conductance (G = 1/R) is:Read the answer and worked solution →The relation between conductivity κ, cell constant (l/A), and conductance G is:Read the answer and worked solution →The molar conductivity Λ_m of an electrolyte solution is defined as:Read the answer and worked solution →As an electrolyte solution is diluted, the **conductivity (κ)** and **molar conductivity (Λ_m)** respectively:Read the answer and worked solution →Given λ°(Ca²⁺) = 119.0 and λ°(Cl⁻) = 76.3 S cm² mol⁻¹, the limiting molar conductivity of CaCl₂ is:Read the answer and worked solution →Given Λ°_m for HCl, NaAc, NaCl = 425.9, 91.0, 126.4 S cm² mol⁻¹ respectively. Calculate Λ°_m for acetic acid (HAc):Read the answer and worked solution →For a weak electrolyte at concentration c, the degree of dissociation α can be approximated as:Read the answer and worked solution →The Faraday constant F = 96500 C mol⁻¹ represents:Read the answer and worked solution →A CuSO₄ solution is electrolysed with 1.5 A for 10 minutes. The mass of copper (M = 63.5) deposited at the cathode is approximately:Read the answer and worked solution →In the electrolysis of **molten** NaCl, the products at the cathode and anode respectively are:Read the answer and worked solution →During electrolysis of **aqueous** NaCl (brine), the products are:Read the answer and worked solution →The electrolyte in a lead storage battery (lead-acid) is approximately:Read the answer and worked solution →In the H₂–O₂ fuel cell used in the Apollo space programme, the electrolyte is:Read the answer and worked solution →Rusting of iron is an electrochemical phenomenon. At the cathodic spot, the reaction is:Read the answer and worked solution →Rust is chemically:Read the answer and worked solution →The de-Broglie wavelength associated with a particle of mass $10^{-6}$ kg with a velocity of $10 \, ms^{-1}$ is:Read the answer and worked solution →

Worked practice questions

In a galvanic cell, the oxidation half-reaction takes place at the:

  1. Cathode, which has positive potential
  2. Both electrodes equally
  3. Anode, which has negative potential
  4. Salt bridge
Show answer and solution

Correct answer: C. Anode, which has negative potential

**Galvanic cell:** **anode = oxidation (negative terminal)**, **cathode = reduction (positive terminal)**. Electrons flow from anode to cathode through the external circuit current flows the opposite way.

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In the standard Daniell cell (Zn|Zn²⁺ || Cu²⁺|Cu) at unit concentrations, the cell EMF is:

  1. 1.86 V
  2. 0.34 V
  3. −0.76 V
  4. 1.10 V
Show answer and solution

Correct answer: D. 1.10 V

E°cell = E°(cathode) − E°(anode) = E°(Cu²⁺/Cu) − E°(Zn²⁺/Zn) = 0.34 − (−0.76) = **+1.10 V**.

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The standard hydrogen electrode (SHE) is assigned a standard electrode potential of:

  1. 0.00 V (by convention)
  2. +1.00 V
  3. +0.76 V
  4. −0.34 V
Show answer and solution

Correct answer: A. 0.00 V (by convention)

SHE — Pt(s) | H₂(g, 1 bar) | H⁺(aq, 1 M) — is assigned **E° = 0.00 V at all temperatures**, serving as the reference for all other standard electrode potentials.

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