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Questions and Answers
What happens at the anode of a galvanic cell?
In the cell notation 𝐶𝑢~(𝑠)~ | 𝐶𝑢^2+^ (1 𝑀) || 𝐴𝑔^+^ (1 𝑀) | 𝐴𝑔~(𝑠)~, which side represents the anode?
What does a double vertical line (||) indicate in cell notation?
How is the cell potential related to standard reduction potentials?
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What is the standard potential of the half-cell reaction usually assigned?
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What does the equation ∆G^0 = -RT ln K represent in relation to cell potentials?
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Which metal acts as the anode in a lithium-manganese battery?
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What type of corrosion is described in the context of galvanic cells?
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Which type of corrosion occurs evenly over a large portion of the surface area of a metal?
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What is defined as the gain of electrons in a chemical reaction?
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In the half-reaction 2Ag^+ + 2e^- → 2Ag(s), which species is the oxidizing agent?
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When copper (Cu) gets oxidized in the reaction Cu(s) → Cu^2+ + 2e^-, what role does Cu play?
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What happens to NH4+ in the galvanic cell when Ag^+ is removed from solution?
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How can standard reduction potentials be used in electrochemistry?
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Which type of corrosion occurs when two different metals contact each other in the presence of an electrolyte?
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What could be a common method to calculate the amount of metal plated in an electrolysis process?
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What is one of the reactants in a zinc-air battery?
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What is the main advantage of nickel-metal-hydride batteries?
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In a lead-acid battery, what material is the anode made of?
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What distinguishes passive electrolysis from active electrolysis?
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Which statement about lithium-ion batteries is correct?
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What is the primary reaction in electrolysis?
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What is a major limitation of traditional batteries?
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What is barrel plating primarily used for?
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Study Notes
Types of Corrosion
- Uniform Corrosion: Occurs evenly across a metal's surface, leading to uniform material loss.
- Galvanic Corrosion: Happens when two dissimilar metals are in contact in the presence of an electrolyte, resulting in accelerated corrosion of the anode metal.
- Crevice Corrosion: Occurs in confined spaces (crevices) where stagnant solutions form, enabling aggressive localized corrosion.
Oxidation and Reduction
- Oxidation: Defined as the loss of electrons from a species.
- Reduction: Defined as the gain of electrons to a species.
- Common half-reaction examples include:
- Silver reduction: ( \text{Ag}^+ + e^- \rightarrow \text{Ag(s)} )
- Copper oxidation: ( \text{Cu(s)} \rightarrow \text{Cu}^{2+} + 2e^- )
Galvanic Cells
- Anode: Electrode where oxidation occurs.
- Cathode: Electrode where reduction occurs.
- Cell Notation: Lists components of the electrochemical cell; phase boundaries indicated by single lines (|) and salt bridges by double lines (||).
- Example notation for a Cu/Ag cell: ( \text{Cu(s)} | \text{Cu}^{2+} (1M) || \text{Ag}^+ (1M) | \text{Ag(s)} )
Cell Potentials
- Cell potentials can be determined through standard electrode potentials.
- Standard hydrogen electrode (SHE) is assigned a potential of 0 volts, used as a reference point.
Standard Reduction Potentials
- Standard reduction potentials help predict the spontaneity of redox reactions using the formula ( E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode} ).
- A higher potential indicates a stronger oxidizing agent and greater tendency for reduction.
Batteries
- Primary Cells: Non-rechargeable batteries; e.g., alkaline batteries with MnO2 and Zn as reactants.
- Secondary Cells: Rechargeable batteries; e.g., nickel-metal-hydride and lead-acid batteries utilized in vehicles.
- Lithium-ion batteries: Feature light materials like lithium and carbon with high energy density.
Electrolysis
- Passive Electrolysis: Employs inert electrodes not involved in the reaction but necessary for electron conduction.
- Active Electrolysis: Involves electrodes that participate in the reaction, altering the composition of the electrolyte.
Current and Charge Calculations
- Fundamental relationships exist between current, charge, and time: ( Q = I \times t ).
- Faraday's constant ( F = 96485 , \text{C mol}^{-1} ) indicates the charge per mole of electrons.
Key Equations
- Gibbs free energy relationship with cell potential: ( \Delta G^\circ = -RT \ln K ), connecting thermodynamics to electrochemistry.
- Stoichiometric calculations for electrolysis: can compute mass change of the products using current, time, and Faraday's laws.
Practical Applications
- Electroplating techniques utilize Faraday's laws to determine current and time required for metal deposition.
- Engineering design increasingly incorporates battery technology, focusing on efficiency and energy density in practical applications, such as electric vehicles.
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Description
Explore the fundamentals of electrochemistry with this quiz, designed for engineering students. You'll describe corrosion types, balance half-reactions, and calculate cell potentials in both standard and nonstandard conditions. Test your understanding of redox reactions and reduction potentials in a practical context.
