Questions and Answers
What is electrochemistry?
The study of production of electricity from energy released during spontaneous chemical reactions and the use of electrical energy to bring about non-spontaneous chemical transformations.
What is a galvanic cell?
What happens when 1.1 V of opposing potential is applied to a galvanic cell?
The reaction stops altogether and no current flows through the cell.
What is the Nernst equation used for?
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What is the significance of molar conductivity (Λm)?
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What type of chemical reactions can generate electrical energy?
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What law concerns the variation of conductivity and molar conductivity with concentration?
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Study Notes
Objectives of Electrochemistry Unit
- Understand the differences between galvanic cells (which produce electrical energy) and electrolytic cells (which require electrical energy to drive non-spontaneous reactions).
- Apply the Nernst equation for calculating the electromotive force (emf) of galvanic cells and define standard potential.
- Derive the relationship between standard potential, Gibbs energy, and the equilibrium constant of cell reactions.
- Define key electrical properties such as resistivity, conductivity, and molar conductivity of ionic solutions.
- Differentiate between ionic electrochemical conductivity and electronic conductivity.
- Learn the methods for measuring the conductivity of electrolytic solutions and calculating their molar conductivity.
- Explain how conductivity and molar conductivity vary with concentration changes.
Key Electrochemical Concepts
- Electrochemistry studies the conversion of chemical energy into electrical energy and vice versa.
- It involves practical applications in energy-efficient and less polluting chemical processes.
- A significant number of essential chemicals, including metals and alkalis like sodium hydroxide, are produced through electrochemical methods.
Importance and Relevance
- Batteries and fuel cells convert chemical energy into electrical energy and are widely used in technology.
- Electrochemical processes are crucial for developing eco-friendly technologies and fostering advancements in science.
- The field has interdisciplinary applications, including communication of sensory signals in living organisms.
Electrochemical Cells
- Daniell cell is an example of a galvanic cell, demonstrating the conversion of chemical energy from redox reactions into electrical energy.
- Reaction in Daniell cell: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s), with a potential of 1.1 V at unit concentrations of Zn²⁺ and Cu²⁺.
- When an opposing potential is applied to a galvanic cell, the cell's current flow stops at 1.1 V but can reverse the reaction if further voltage is applied.
Conductivity and Molar Conductivity
- Molar conductivity (Λm) is defined as molar conductivity at infinite dilution.
- Kohlrausch's law applies to understand how conductivities change and has various applications in electrochemistry.
- Conductivity and molar conductivity vary based on concentration, impacting the efficiency of electrochemical processes.
Corrosion and Electrochemistry
- Corrosion is treated as an electrochemical process, highlighting the practical importance of studying electrochemistry.
- Understanding electrochemical principles helps in addressing issues of material degradation and enhancing the longevity of devices.
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Description
Test your understanding of electrochemical cells with this quiz. You will explore the differences between galvanic and electrolytic cells, and how chemical reactions can produce electrical energy. Engage with key concepts and enhance your knowledge in electrochemistry.
