Practice Standard Electrode Potential Values and their Significance - 8.4.3 | Chapter 7: Redox Processes | IB Grade 12-Chemistry
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8.4.3 - Standard Electrode Potential Values and their Significance

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Learning

Practice Questions

Test your understanding with targeted questions related to the topic.

Question 1

Easy

What does a positive standard electrode potential (E°) indicate?

💡 Hint: Think about which substance is likely to gain electrons.

Question 2

Easy

What is the standard electrode potential of the SHE?

💡 Hint: This is our reference point for other electrodes.

Practice 4 more questions and get performance evaluation

Interactive Quizzes

Engage in quick quizzes to reinforce what you've learned and check your comprehension.

Question 1

What is the significance of a positive standard electrode potential (E°)?

  • It indicates a stronger reducing agent
  • It indicates a stronger oxidizing agent
  • It is irrelevant

💡 Hint: Think about the role of oxidizing agents in redox reactions.

Question 2

True or False: E°_cell must always be positive for a reaction to occur.

  • True
  • False

💡 Hint: Consider what happens in electrolytic cells.

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Challenge Problems

Push your limits with challenges.

Question 1

Consider two half-reactions: A²⁺ + 2e⁻ ⇌ A(s) E° = +0.76 V and B²⁺ + 2e⁻ ⇌ B(s) E° = -0.44 V. Which species would act as the reducing agent if combined in a galvanic cell?

💡 Hint: Compare E° values to determine the roles of oxidizing and reducing agents.

Question 2

Calculate the cell potential and determine spontaneity of the reaction between Ag⁺ and Cu with E° values of +0.80 V and -0.34 V respectively.

💡 Hint: Follow the formula for E°_cell using cathode and anode values.

Challenge and get performance evaluation