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Questions and Answers
What type of electrochemical cell uses the energy released during a spontaneous redox reaction?
What type of electrochemical cell uses the energy released during a spontaneous redox reaction?
Anode is located on the right-hand side of a galvanic cell.
Anode is located on the right-hand side of a galvanic cell.
False
What is the significance of EMF in a cell?
What is the significance of EMF in a cell?
Electromotive force indicates the feasibility of the cell operation.
A galvanic cell is also called a _____ cell.
A galvanic cell is also called a _____ cell.
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What occurs at the cathode during the electrolysis of molten NaCl?
What occurs at the cathode during the electrolysis of molten NaCl?
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Which of the following represents the half cell reaction at the anode during the electrolysis of molten NaCl?
Which of the following represents the half cell reaction at the anode during the electrolysis of molten NaCl?
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What happens during the electrolysis of water?
What happens during the electrolysis of water?
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The standard reduction potentials for Cd and Cu2+ are _____ V and _____ V respectively, where Cd is -0.40 V and Cu2+ is 0.34 V.
The standard reduction potentials for Cd and Cu2+ are _____ V and _____ V respectively, where Cd is -0.40 V and Cu2+ is 0.34 V.
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What is generated at the cathode in a Galvanic cell during a redox reaction?
What is generated at the cathode in a Galvanic cell during a redox reaction?
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Study Notes
Electrochemical Cells
- Devices that generate electricity from spontaneous redox reactions or use electricity to drive non-spontaneous redox reactions.
- Comprise two electrodes (anode and cathode) and an electrolyte.
- Commonly linked by a metal wire; copper is often used.
Types of Electrochemical Cells
- Galvanic (Voltaic) Cells: Utilize energy from spontaneous redox reactions (ΔG < 0) to produce electricity.
- Named after Alessandro Volta, the inventor of this cell type.
Galvanic Cell Representation
- Anode (oxidation) is on the left; cathode (reduction) is on the right.
- Example: Zn|Zn(NO3)2 (1M) || Cu(NO3)2 (1M)|Cu demonstrates oxidation and reduction processes.
Flow of Electrons and Current
- Electrons flow from anode to cathode; current flows in the opposite direction.
- Cell feasibility: feasible if EMF is positive; not feasible if EMF is negative.
Calculating Standard EMF of a Cell
- Standard EMF can be calculated using the standard reduction potentials of the involved metals.
- Example calculation involves Zn (-0.76 V) and Ag (+0.80 V) to determine overall EMF.
Nernst Equation and Electrochemical Calculations
- Essential for calculating cell potentials under non-standard conditions.
- Used to determine equilibrium constants and analyze half-cell reactions.
Electrolysis of Molten NaCl
- Na+ ions are reduced to Na at the cathode, and Cl- ions are oxidized to Cl2 at the anode.
- The electrolysis process occurs at approximately 801 °C using inert electrodes.
Inert Electrodes in Electrolysis
- Inert electrodes, like graphite rods, do not participate in the chemical reactions.
- Power supply is needed to drive electron movement from anode to cathode.
Electrolysis of Water
- Involves a pair of inert electrodes submerged in water; applying voltage promotes the decomposition of water into hydrogen and oxygen gases.
Key Reactions in Electrochemical Processes
- For electrolysis of NaCl: 2 NaCl (l) → 2 Na (l) + Cl2 (g) at the anode.
- Importance of maintaining ion movement during electrolysis to ensure continuous reactions.
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Description
This quiz covers Module 4 of Engineering Chemistry BCHY101L, focusing on energy devices. Topics include electrochemical cells, electrode materials, lithium-ion batteries, supercapacitors, fuel cells, and solar cells. Test your knowledge on these essential technologies that power various applications in modern engineering.
