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Questions and Answers
What happens at the anode of a galvanic cell?
What happens at the anode of a galvanic cell?
- No reaction occurs.
- Oxidation occurs. (correct)
- Reduction occurs.
- Both oxidation and reduction occur.
In the cell notation 𝐶𝑢~(𝑠)~ | 𝐶𝑢^2+^ (1 𝑀) || 𝐴𝑔^+^ (1 𝑀) | 𝐴𝑔~(𝑠)~, which side represents the anode?
In the cell notation 𝐶𝑢~(𝑠)~ | 𝐶𝑢^2+^ (1 𝑀) || 𝐴𝑔^+^ (1 𝑀) | 𝐴𝑔~(𝑠)~, which side represents the anode?
- Neither side.
- Both sides.
- Left side. (correct)
- Right side.
What does a double vertical line (||) indicate in cell notation?
What does a double vertical line (||) indicate in cell notation?
- A phase boundary.
- Oxidation reaction.
- An electrode.
- A salt bridge. (correct)
How is the cell potential related to standard reduction potentials?
How is the cell potential related to standard reduction potentials?
What is the standard potential of the half-cell reaction usually assigned?
What is the standard potential of the half-cell reaction usually assigned?
What does the equation ∆G^0 = -RT ln K represent in relation to cell potentials?
What does the equation ∆G^0 = -RT ln K represent in relation to cell potentials?
Which metal acts as the anode in a lithium-manganese battery?
Which metal acts as the anode in a lithium-manganese battery?
What type of corrosion is described in the context of galvanic cells?
What type of corrosion is described in the context of galvanic cells?
Which type of corrosion occurs evenly over a large portion of the surface area of a metal?
Which type of corrosion occurs evenly over a large portion of the surface area of a metal?
What is defined as the gain of electrons in a chemical reaction?
What is defined as the gain of electrons in a chemical reaction?
In the half-reaction 2Ag^+ + 2e^- → 2Ag(s), which species is the oxidizing agent?
In the half-reaction 2Ag^+ + 2e^- → 2Ag(s), which species is the oxidizing agent?
When copper (Cu) gets oxidized in the reaction Cu(s) → Cu^2+ + 2e^-, what role does Cu play?
When copper (Cu) gets oxidized in the reaction Cu(s) → Cu^2+ + 2e^-, what role does Cu play?
What happens to NH4+ in the galvanic cell when Ag^+ is removed from solution?
What happens to NH4+ in the galvanic cell when Ag^+ is removed from solution?
How can standard reduction potentials be used in electrochemistry?
How can standard reduction potentials be used in electrochemistry?
Which type of corrosion occurs when two different metals contact each other in the presence of an electrolyte?
Which type of corrosion occurs when two different metals contact each other in the presence of an electrolyte?
What could be a common method to calculate the amount of metal plated in an electrolysis process?
What could be a common method to calculate the amount of metal plated in an electrolysis process?
What is one of the reactants in a zinc-air battery?
What is one of the reactants in a zinc-air battery?
What is the main advantage of nickel-metal-hydride batteries?
What is the main advantage of nickel-metal-hydride batteries?
In a lead-acid battery, what material is the anode made of?
In a lead-acid battery, what material is the anode made of?
What distinguishes passive electrolysis from active electrolysis?
What distinguishes passive electrolysis from active electrolysis?
Which statement about lithium-ion batteries is correct?
Which statement about lithium-ion batteries is correct?
What is the primary reaction in electrolysis?
What is the primary reaction in electrolysis?
What is a major limitation of traditional batteries?
What is a major limitation of traditional batteries?
What is barrel plating primarily used for?
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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