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Karnataka PUC II Electrochemistry — practice questions — page 3

Explore 95 free Electrochemistry questions in Karnataka PUC II Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Electrochemistry questions and exercises with answers

Showing questions 61–90 of 95.

The standard electrode potential of the Standard Hydrogen Electrode (SHE) is defined as:Read the answer and worked solution →The Daniell cell (Zn-Cu) has E°cell = +1.10 V. Calculate ΔG° (F = 96500 C/mol):Read the answer and worked solution →Faraday's first law of electrolysis states that the mass deposited is:Read the answer and worked solution →The byproduct of a hydrogen-oxygen fuel cell (used in space + electric cars) is:Read the answer and worked solution →Order these electrodes by standard potential, lowest firstRead the answer and worked solution →True or false: conductivity on dilutionRead the answer and worked solution →Strong electrolyte or weak electrolyte?Read the answer and worked solution →Match each relation to what it linksRead the answer and worked solution →True or false: cells and electrodesRead the answer and worked solution →Tap every statement true of a galvanic cellRead the answer and worked solution →Assertion and reasonRead the answer and worked solution →Two are true, one is notRead the answer and worked solution →Which quantity is being described?Read the answer and worked solution →True or false: batteries, fuel cells and corrosionRead the answer and worked solution →True or false: the standard scaleRead the answer and worked solution →Galvanic or electrolytic cell?Read the answer and worked solution →True or false: electrochemistryRead the answer and worked solution →Match each electrode to the potential your syllabus givesRead the answer and worked solution →Assertion and reason: potentialsRead the answer and worked solution →Reading the definitions backRead the answer and worked solution →Kohlrausch's lawRead the answer and worked solution →Which half-reaction from the notes represents reduction?Read the answer and worked solution →The Nernst equation at 25°C for a cell reaction is:Read the answer and worked solution →Tap every factor conductivity depends onRead the answer and worked solution →In a Daniell cell, $\mathrm{Zn} | \mathrm{Zn}^{2+}(aq) \,||\, \mathrm{Cu}^{2+}(aq) | \mathrm{Cu}$, the standard EMF is calculated as:Read the answer and worked solution →NEET · Chemistry · Galvanic vs Electrolytic CellRead the answer and worked solution →Order the steps: find a standard cell potentialRead the answer and worked solution →Spot the one that does not belongRead the answer and worked solution →Flip and pair: symbol with meaningRead the answer and worked solution →Complete the dilution behaviourRead the answer and worked solution →

Worked practice questions

The standard electrode potential of the Standard Hydrogen Electrode (SHE) is defined as:

  1. $+1.10$ V (the Daniell cell value)
  2. $0$ V exactly (the universal reference)
  3. $+0.34$ V (the Cu electrode value)
  4. $-0.76$ V (the Zn electrode value)
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Correct answer: B. $0$ V exactly (the universal reference)

SHE is the UNIVERSAL REFERENCE with E° defined as 0 V exactly. All other electrode potentials are measured relative to SHE. Cu/Cu²⁺ = +0.34 V; Zn/Zn²⁺ = −0.76 V.

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The Daniell cell (Zn-Cu) has E°cell = +1.10 V. Calculate ΔG° (F = 96500 C/mol):

  1. $-106 kJ$ (using wrong n value)
  2. $-53 kJ$ (using n = 1)
  3. $+212 kJ$ (positive sign incorrect)
  4. $-212 kJ/mol$ (using n = 2)
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Correct answer: D. $-212 kJ/mol$ (using n = 2)

ΔG° = −nFE° = −2 × 96500 × 1.10 = −212,300 J/mol = −212 kJ/mol. Negative ΔG° confirms spontaneous reaction (galvanic cell works). n = 2 for Zn → Zn²⁺ + 2e⁻.

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Faraday's first law of electrolysis states that the mass deposited is:

  1. Inversely proportional to the charge passed (Q)
  2. Directly proportional to the charge passed (Q)
  3. Independent of the molar mass of the substance
  4. Proportional to the square of the current passed
Show answer and solution

Correct answer: B. Directly proportional to the charge passed (Q)

**Faraday's 1st law:** m = QM/(nF), so mass deposited is DIRECTLY PROPORTIONAL to charge Q = It. Higher current OR longer time → more mass deposited.

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