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JEE Main Electrochemistry — practice questions — page 3

Explore 114 free Electrochemistry questions in JEE Main 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 114.

Going from top to bottom of the table, the electrode potential:Read the answer and worked solution →A negative standard potential marks a reducing agent that is:Read the answer and worked solution →In the Daniell cell, zinc dissolves at the anode and copper:Read the answer and worked solution →The two portions of a galvanic cell are also called:Read the answer and worked solution →The electrolytes of the two half-cells are joined by a:Read the answer and worked solution →True or false on electrochemistryRead the answer and worked solution →Quick picks on cellsRead the answer and worked solution →Anode or cathodeRead the answer and worked solution →Match each part to its jobRead the answer and worked solution →Oxidising or reducing agentRead the answer and worked solution →Trace the Daniell cellRead the answer and worked solution →Fill the gaps on electrochemistryRead the answer and worked solution →Spot the one that does not fitRead the answer and worked solution →For a cell reaction with $E^\circ_\text{cell} = +0.59\,\text{V}$ and $n = 2$, the equilibrium constant $K$ at $298\,\text{K}$ is approximately:Read the answer and worked solution →Complete the standard cell potential relationRead the answer and worked solution →Complete the thermodynamic linksRead the answer and worked solution →What the Nernst equation is forRead the answer and worked solution →The situation in which the charge buildup near the Zn rod prevents further oxidation is called:Read the answer and worked solution →Which half-reaction from the given notes represents oxidation?Read the answer and worked solution →Which of the following is classified as a secondary (rechargeable) cell?Read the answer and worked solution →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 →

Worked practice questions

Going from top to bottom of the table, the electrode potential:

  1. Increases
  2. Stays same
  3. Goes to zero
  4. Decreases
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Correct answer: D. Decreases

1. The table is ordered by standard electrode potential. 2. The value falls as one reads downwards. 3. Oxidising power falls with it and reducing power rises. _Source: syllabus Chemistry Part I, Chapter 3, Electrochemistry._

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A negative standard potential marks a reducing agent that is:

  1. Stronger
  2. Weaker
  3. Absent
  4. Neutral
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Correct answer: A. Stronger

1. The comparison is against the hydrogen couple. 2. A negative value places the couple below hydrogen. 3. Such a couple is a stronger reducing agent than hydrogen. _Source: syllabus Chemistry Part I, Chapter 3, Electrochemistry._

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In the Daniell cell, zinc dissolves at the anode and copper:

  1. Stays free
  2. Deposits
  3. Dissolves
  4. Evaporates
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Correct answer: B. Deposits

1. Zinc is oxidised, so the zinc electrode loses material. 2. Copper ions are reduced at the other electrode. 3. So copper is deposited on the cathode. _Source: syllabus Chemistry Part I, Chapter 3, Electrochemistry._

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