Electrochemistry Basics - Exam-Ready Higher Difficulty Problems

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Electrochemistry Basics - Higher Difficulty Problems

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Electrochemistry Basics - Higher Difficulty Problems MCQ & Objective Questions

Understanding "Electrochemistry Basics - Higher Difficulty Problems" is crucial for students aiming to excel in their exams. These concepts form the foundation of many important topics in chemistry, making it essential to practice MCQs and objective questions. Engaging with these practice questions not only enhances your knowledge but also boosts your confidence, helping you score better in your exams.

What You Will Practise Here

Fundamental concepts of electrochemistry including oxidation and reduction reactions.
Understanding electrochemical cells and their components.
Calculating standard electrode potentials and their significance.
Application of Nernst equation in various scenarios.
Analyzing galvanic and electrolytic cells through diagrams and equations.
Exploring Faraday's laws of electrolysis and their applications.
Solving complex numerical problems related to electrochemical principles.

Exam Relevance

Electrochemistry is a significant topic in various examinations such as CBSE, State Boards, NEET, and JEE. Questions often focus on the application of concepts in real-world scenarios, calculations involving cell potentials, and understanding the principles behind electrolysis. Familiarity with common question patterns, such as numerical problems and conceptual MCQs, is vital for effective exam preparation.

Common Mistakes Students Make

Confusing oxidation and reduction processes, leading to incorrect answers.
Misapplying the Nernst equation due to misunderstanding its components.
Overlooking the significance of standard electrode potentials in problem-solving.
Failing to interpret electrochemical cell diagrams accurately.
Neglecting units in calculations, which can result in errors in numerical answers.

FAQs

Question: What are the key components of an electrochemical cell?
Answer: An electrochemical cell consists of two electrodes (anode and cathode), an electrolyte, and a salt bridge.

Question: How does the Nernst equation help in electrochemistry?
Answer: The Nernst equation allows us to calculate the cell potential under non-standard conditions, providing insights into the reaction's spontaneity.

Now is the time to enhance your understanding of electrochemistry! Dive into our practice MCQs and test your knowledge on important Electrochemistry Basics - Higher Difficulty Problems questions for exams. Your success starts with practice!

Q. For a redox reaction, if the standard reduction potentials are E°(A/B) = 0.80 V and E°(C/D) = 0.40 V, which species is the stronger oxidizing agent?

A. A
B. B
C. C
D. D

Solution

The stronger oxidizing agent is the one with the higher reduction potential. Here, A/B has a higher E° than C/D.

Correct Answer: A — A

Q. If the concentration of reactants in a redox reaction is doubled, how does it affect the cell potential according to the Nernst equation?

A. Increases
B. Decreases
C. Remains the same
D. Depends on temperature

Solution

Doubling the concentration of reactants increases Q, which decreases E according to the Nernst equation.

Correct Answer: B — Decreases

Q. In a concentration cell, if the concentration of the anode is 0.1 M and the cathode is 1 M, what is the cell potential at 25°C?

A. 0.059 V
B. 0.118 V
C. 0.059 log(10)
D. 0.118 log(10)

Solution

E = (0.059 V/n) * log([Cathode]/[Anode]) = (0.059 V/2) * log(1/0.1) = 0.059 V * 1 = 0.059 V.

Correct Answer: B — 0.118 V

Q. In a concentration cell, if the concentration of the anode is 0.1 M and the cathode is 1.0 M, what is the cell potential at 25°C?

A. 0.059 V
B. 0.118 V
C. 0.059 log(10)
D. 0.118 log(10)

Solution

E = (0.059 V/n) * log([Cathode]/[Anode]) = (0.059 V/2) * log(10) = 0.059 V.

Correct Answer: B — 0.118 V

Q. In a Daniell cell, what is the role of the salt bridge?

A. To provide a pathway for electrons
B. To maintain charge neutrality
C. To increase the cell potential
D. To facilitate ion exchange

Solution

The salt bridge maintains charge neutrality by allowing ions to flow between the two half-cells.

Correct Answer: B — To maintain charge neutrality

Q. In a Daniell cell, which species is reduced?

A. Zn
B. Cu²⁺
C. Zn²⁺
D. Cu

Solution

In a Daniell cell, Cu²⁺ is reduced to Cu at the cathode.

Correct Answer: B — Cu²⁺

Q. In a galvanic cell, if the anode reaction is Zn → Zn²⁺ + 2e⁻, what is the half-reaction at the cathode if Cu²⁺ is reduced?

A. Cu + 2e⁻ → Cu²⁺
B. Cu²⁺ + 2e⁻ → Cu
C. Cu²⁺ → Cu + 2e⁻
D. Cu → Cu²⁺ + 2e⁻

Solution

The cathode reaction involves the reduction of Cu²⁺ to Cu: Cu²⁺ + 2e⁻ → Cu.

Correct Answer: B — Cu²⁺ + 2e⁻ → Cu

Q. In a redox reaction, if the oxidation state of manganese changes from +7 to +2, how many electrons are gained?

A. 5
B. 3
C. 2
D. 7

Solution

The change from +7 to +2 indicates a gain of 5 electrons (7 - 2 = 5).

Correct Answer: C — 2

Q. What is the effect of increasing temperature on the cell potential of an electrochemical cell?

A. Increases cell potential
B. Decreases cell potential
C. No effect
D. Depends on the reaction

Solution

The effect of temperature on cell potential depends on the reaction's enthalpy and entropy changes.

Correct Answer: D — Depends on the reaction

Q. What is the effect of increasing temperature on the cell potential of an electrochemical reaction?

A. Increases cell potential.
B. Decreases cell potential.
C. No effect on cell potential.
D. Depends on the reaction.

Solution

The effect of temperature on cell potential depends on the reaction's enthalpy and entropy changes.

Correct Answer: D — Depends on the reaction.

Q. What is the Nernst equation used for calculating the cell potential under non-standard conditions?

A. E = E° - (RT/nF)ln(Q)
B. E = E° + (RT/nF)ln(Q)
C. E = E° - (nF/RT)ln(Q)
D. E = E° + (nF/RT)ln(Q)

Solution

The Nernst equation is E = E° - (RT/nF)ln(Q), where R is the gas constant, T is temperature, n is moles of electrons, and F is Faraday's constant.

Correct Answer: A — E = E° - (RT/nF)ln(Q)

Q. What is the relationship between Gibbs free energy (ΔG) and cell potential (E) in an electrochemical cell?

A. ΔG = -nFE
B. ΔG = nFE
C. ΔG = -E/nF
D. ΔG = E/nF

Solution

The relationship is given by ΔG = -nFE, where n is the number of moles of electrons and F is Faraday's constant.

Correct Answer: A — ΔG = -nFE

Q. What is the relationship between Gibbs free energy change (ΔG) and cell potential (E) in electrochemistry?

A. ΔG = -nFE
B. ΔG = nFE
C. ΔG = -E/nF
D. ΔG = E/nF

Solution

The relationship is given by ΔG = -nFE, where n is the number of moles of electrons and F is Faraday's constant.

Correct Answer: A — ΔG = -nFE

Q. What is the standard cell potential (E°) for a galvanic cell composed of a zinc electrode and a copper electrode?

A. 0.34 V
B. 1.10 V
C. 0.76 V
D. 1.96 V

Solution

E° = E°(Cu²⁺/Cu) - E°(Zn²⁺/Zn) = 0.34 V - (-0.76 V) = 1.10 V.

Correct Answer: B — 1.10 V

Q. What is the standard electrode potential for the reduction of Ag⁺ to Ag?

A. 0.80 V
B. 0.46 V
C. 0.34 V
D. 0.00 V

Solution

The standard electrode potential for the reduction of Ag⁺ to Ag is 0.80 V.

Correct Answer: B — 0.46 V

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