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9. Consider the reduction of 10-3 mole/cm³ Cu²+ to Cut which has a diffusion limited current density of -9.2 mA/cm², for a diffusion boundary layer thickness of 10-2 cm and an electrolyte diffusivity, D, of Cu²+ of 1 x 10-6 cm²/s. Determine the diffusion overvoltage at a current density of -4.6 mA/cm². a. -1.78 V b. -0.178 V c. -0.0178 V d. -0.0018 V

9. Consider the reduction of 10-3 mole/cm³ Cu²+ to Cut which has a diffusion limited current density of -9.2 mA/cm², for a diffusion boundary layer thickness of 10-2 cm and an electrolyte diffusivity, D, of Cu²+ of 1 x 10-6 cm²/s. Determine the diffusion overvoltage at a current density of -4.6 mA/cm². a. -1.78 V b. -0.178 V c. -0.0178 V d. -0.0018 V

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Transcription for Educational Website** --- **7. Consider the following current densities:** a. 3.0 mA/cm² b. 0.30 mA/cm² c. 0.03 mA/cm² d. 0.003 mA/cm² --- **8. If the standard free energy of formation of Az³⁺ is 51,500 calories/mole, determine the standard potential for the reaction, Az³⁺ + 3e⁻ = Az. *Az is a newly discovered element.** a. +0.744 V b. -0.744 V c. +1.110 V d. -1.110 V --- **9. Consider the reduction of 10⁻³ mole/cm³ Cu²⁺ to Cu⁺ which has a diffusion-limited current density of -9.2 mA/cm², for a diffusion boundary layer thickness of 10⁻² cm and an electrolyte diffusivity, D, of Cu²⁺ of 1 x 10⁻⁶ cm²/s. Determine the diffusion overvoltage at a current density of -4.6 mA/cm².** a. -1.78 V b. -0.178 V c. -0.0178 V d. -0.0018 V --- **10. Consider the battery below containing 1M CuSO₄ and 1M ZnSO₄ which is capable of delivering a voltage of 1.104 V. You need this voltage to operate your device. Eventually, the battery will stop functioning as the voltage will drop to near zero. What can you do to extend the lifetime of the battery?** --- **Diagram Explanation:** The diagram shows a galvanic cell setup: - **Copper (cathode)**: The left side contains a copper electrode submerged in a CuSO₄ solution. - **Zinc (anode)**: The right side contains a zinc electrode submerged in a ZnSO₄ solution. - **Salt bridge**: Positioned between the two solutions, it allows the flow of ions without mixing the solutions directly. - **Voltmeter**: Connected across the electrodes to measure the voltage. This setup illustrates the basic operation of a galvanic cell, where chemical energy is converted into electrical energy. --- This transcription provides a detailed explanation of the concepts, enhancing
Transcribed Image Text:**Transcription for Educational Website** --- **7. Consider the following current densities:** a. 3.0 mA/cm² b. 0.30 mA/cm² c. 0.03 mA/cm² d. 0.003 mA/cm² --- **8. If the standard free energy of formation of Az³⁺ is 51,500 calories/mole, determine the standard potential for the reaction, Az³⁺ + 3e⁻ = Az. *Az is a newly discovered element.** a. +0.744 V b. -0.744 V c. +1.110 V d. -1.110 V --- **9. Consider the reduction of 10⁻³ mole/cm³ Cu²⁺ to Cu⁺ which has a diffusion-limited current density of -9.2 mA/cm², for a diffusion boundary layer thickness of 10⁻² cm and an electrolyte diffusivity, D, of Cu²⁺ of 1 x 10⁻⁶ cm²/s. Determine the diffusion overvoltage at a current density of -4.6 mA/cm².** a. -1.78 V b. -0.178 V c. -0.0178 V d. -0.0018 V --- **10. Consider the battery below containing 1M CuSO₄ and 1M ZnSO₄ which is capable of delivering a voltage of 1.104 V. You need this voltage to operate your device. Eventually, the battery will stop functioning as the voltage will drop to near zero. What can you do to extend the lifetime of the battery?** --- **Diagram Explanation:** The diagram shows a galvanic cell setup: - **Copper (cathode)**: The left side contains a copper electrode submerged in a CuSO₄ solution. - **Zinc (anode)**: The right side contains a zinc electrode submerged in a ZnSO₄ solution. - **Salt bridge**: Positioned between the two solutions, it allows the flow of ions without mixing the solutions directly. - **Voltmeter**: Connected across the electrodes to measure the voltage. This setup illustrates the basic operation of a galvanic cell, where chemical energy is converted into electrical energy. --- This transcription provides a detailed explanation of the concepts, enhancing
Expert Solution
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9. To solve this problem, we can use the following equation:

ηd=RT/(nF)ln[1−(j/jlim)]

where:

  • η_d is the diffusion overvoltage
  • R is the universal gas constant
  • T is the temperature in Kelvin
  • n is the number of electrons transferred in the electrochemical reaction
  • F is Faraday's constant
  • j is the current density
  • j_lim is the limiting current density
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