Electrochemistry: Fundamentals and Applications
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Questions and Answers

What causes the development of a potential difference across the barrier in a solution?

  • The equal mobility of H^+^ and Cl^−^ ions
  • The greater mobility of H^+^ ions compared to Cl^−^ ions (correct)
  • The concentration of Cl^−^ ions being higher than H^+^ ions
  • The negative charge of the H^+^ ions in the solution
  • What is the term for the steady state potential difference that exists when both H^+^ and Cl^−^ ions cross over at the same rate?

  • Osmotic potential
  • Standard Electrode Potential
  • Electrochemical potential
  • Liquid Junction Potential (correct)
  • What is the purpose of using a salt bridge filled with ions of similar mobilities in an electrochemical cell?

  • To improve the efficiency of the cell (correct)
  • To decrease the temperature of the system
  • To promote the oxidation of metals
  • To increase the concentration of H^+^ ions
  • Under what conditions does the Nernst Equation allow for calculations of electrochemical cell potential?

    <p>At varying concentrations and gas pressures</p> Signup and view all the answers

    In the context of electrochemical cells, what happens to the electrical energy when overcoming the liquid junction potential?

    <p>Some of it is wasted</p> Signup and view all the answers

    What occurs at the cathode in an electrochemical cell?

    <p>Reduction of metal cations</p> Signup and view all the answers

    Which statement accurately describes the oxidation process in this electrochemical system?

    <p>Zn is converted into Zn^2+.</p> Signup and view all the answers

    What is the role of the salt bridge in an electrochemical cell?

    <p>To allow ions to flow and prevent charge build-up</p> Signup and view all the answers

    Which metal is undergoing reduction in the reaction involving Cu and Zn?

    <p>Cu</p> Signup and view all the answers

    What happens to the equilibrium when an electron is added to the Cu half-cell?

    <p>It shifts to the left</p> Signup and view all the answers

    What is the result when all Zn metal is oxidized in the electrochemical cell?

    <p>The reaction will halt.</p> Signup and view all the answers

    How can the potential for non-standard half-cells be determined?

    <p>Using the Nernst equation</p> Signup and view all the answers

    In an electrochemical cell, the amount of oxidation at the anode is equal to what?

    <p>The amount of reduction at the cathode</p> Signup and view all the answers

    What describes the state of equilibrium at the metal-electrolyte interface?

    <p>The rate of cations dissolving matches the rate of cations depositing.</p> Signup and view all the answers

    Which equation relates the potentials of an electrochemical cell to temperature and concentration?

    <p>Nernst equation</p> Signup and view all the answers

    What does the charge on the metal side of the interface depend on?

    <p>The tendency of the metal to form cations</p> Signup and view all the answers

    Which of the following describes the nature of metals at the metal-electrolyte interface?

    <p>Metals consist of fixed cations and free-moving electrons.</p> Signup and view all the answers

    What occurs when two species in different phases are in equilibrium?

    <p>The Gibbs energy of the species is equal in both phases</p> Signup and view all the answers

    What does the exchange current density indicate in electrochemical kinetics?

    <p>The rate of electron transfer in an electrochemical reaction.</p> Signup and view all the answers

    What is the term for the Gibbs energy per mole of an uncharged species?

    <p>Chemical Potential</p> Signup and view all the answers

    Which type of voltammetry involves the potential being changed linearly with time?

    <p>Linear sweep voltammetry</p> Signup and view all the answers

    What additional factor contributes to the change in energy when a charged species moves across an interface?

    <p>Electrochemical potential difference</p> Signup and view all the answers

    What leads to a build-up of positive charges on the metal during equilibrium?

    <p>Cations escaping from the solution and depositing onto the metal</p> Signup and view all the answers

    What is one main function of Pourbaix diagrams in corrosion studies?

    <p>To provide a visual representation of corrosion potentials.</p> Signup and view all the answers

    What characteristic of batteries reflects their ability to store energy over time?

    <p>Capacity</p> Signup and view all the answers

    What is represented by the symbol μ in the context of chemical potential?

    <p>Chemical potential in J mol^-1</p> Signup and view all the answers

    Which statement about fuel cells is correct?

    <p>Fuel cells require a source of hydrogen fuel for their reactions.</p> Signup and view all the answers

    Which of the following species would likely prefer to be in a metallic state?

    <p>More noble metals like Au and Ag</p> Signup and view all the answers

    The equation ∆G = μsolution − μsolid describes which type of change?

    <p>Chemical reaction energy change</p> Signup and view all the answers

    What happens to the Fermi Level when a more positive potential is applied to the electrode?

    <p>It decreases, causing a shift towards oxidation.</p> Signup and view all the answers

    What does the exchange current density represent in an electrochemical system?

    <p>The equal rates of oxidation and reduction at equilibrium.</p> Signup and view all the answers

    When the electrode potential is decreased from +0.77 V to +0.5 V, which reaction is favored?

    <p>Reduction, leading to a decrease in Fe^3+ concentration.</p> Signup and view all the answers

    At equilibrium, what is the condition of net current density?

    <p>It equals zero.</p> Signup and view all the answers

    What is the effect of making the electrode potential more negative?

    <p>It adds energy to the electrons at the electrode.</p> Signup and view all the answers

    In the context of electron transfer, what is the significance of the Nernst Equation?

    <p>It determines the equilibrium potential for given concentrations.</p> Signup and view all the answers

    What are the oxidation and reduction processes characterized by when considering electron movement?

    <p>Electrons enter the surface for oxidation and leave for reduction.</p> Signup and view all the answers

    What is the effect of reaching equilibrium between the Fermi Level and the energy levels of ions in solution?

    <p>No net change occurs in the system.</p> Signup and view all the answers

    What does it indicate when both E_cell is positive and ΔG is negative?

    <p>The reaction is spontaneous as written.</p> Signup and view all the answers

    In the Nernst equation, what is the significance of concentrations being in mol dm^-3?

    <p>It allows for the proper calculation of cell potential under non-standard conditions.</p> Signup and view all the answers

    When using the Nernst equation, which of the following assumptions is made about solids?

    <p>They have an effective concentration of 1.</p> Signup and view all the answers

    What is the relationship between ΔS and E_cell when temperature changes?

    <p>The sign of ΔS can sometimes be predicted from E_cell changes.</p> Signup and view all the answers

    In a cell composed of Cu|Cu^2+ and Ag^+|Ag, what happens to the copper ions during the reaction?

    <p>They are reduced to copper metal.</p> Signup and view all the answers

    Which condition does not affect the effective concentration used in the Nernst equation?

    <p>Solids such as metals.</p> Signup and view all the answers

    Which parameter can be estimated by measuring how E_cell changes over a short temperature range?

    <p>ΔH and ΔS.</p> Signup and view all the answers

    What determines the spontaneity of a reaction based on E_cell and ΔG?

    <p>Spontaneity is indicated by a positive E_cell and a negative ΔG.</p> Signup and view all the answers

    Study Notes

    Electrochemistry: Fundamentals and Applications

    • The metal-electrolyte interface. Electrochemical equilibrium and electrochemical potential.
    • Electrochemical half-cells and cells. Types of electrodes, electrode and cell potentials. Nernst Equation. Liquid junction potential. Thermodynamic aspects of electrochemistry.
    • Electrode kinetics and overpotential, the Butler-Volmer equation.
    • Tafel equation. Exchange current density and mass transfer.
    • Linear sweep and cyclic voltammetry.
    • Corrosion and Pourbaix diagrams. Applications of Pourbaix diagrams. Evaluation of the Gibbs energy change in the corrosion reaction. Corrosion prevention and control.
    • Batteries: battery characteristics; voltage, current, capacity. Storage density and cycle life. Examples: lead-acid, Ni-Cd, Ni-MH, and Li-ion batteries.
    • Introduction to Fuel Cells: reactions and cell design. Source of H₂ fuel. Applications and future prospects.
    • Assessment details: Online class test worth 10% of the module mark. One question in the December exam worth 15% of the module mark.

    Equilibrium Electrochemistry

    • Metals consist of fixed cations in a lattice with free electrons that can move through the lattice.
    • Solutions contain ions that move through the solution, carrying positive and negative charges. Cations (positive ions) move to the cathode during electrolysis; anions (negative ions) move to the anode.
    • When a metal and a solution of its ions are in contact, two processes can occur:
    • The metal can initially dissolve, releasing cations into solution
    • Initial deposition of metal ions onto the metal occurs, depositing cations onto the metal surface, forming a net positive charge on the metal, and a net negative charge on the solution side of the interface.
    • Equilibrium will be quickly reached when the rate of metal cations moving into solution is the same as the rate of cations depositing back onto the metal.
    • The charge on the metal side of the interface depends on the metal.
    • At equilibrium, a stable interfacial potential difference (ΔΦ) will exist across the metal/solution interface.

    Chemical Potential

    • The Gibbs energy per mole of an uncharged species is called its chemical potential.
    • If two species in different phases, such as a metal and ions in solution, are in equilibrium with each other, if a species moves from the solid to the solution, there will be a change in Gibbs energy. This ΔG describes the electrochemical process, accounting for charge transfer.

    Electrochemical Potential

    • If a charged species moves across an interface where there is an electrical potential difference, this will additionally contribute to the change in energy.
    • The electrochemical potential is defined to include all these effects
    • chemical potential of the species, μ
    • Galvani potential of species, φ
    • charge of the species, n
    • Faraday constant, F

    Cell Notation

    • The vertical line represents a phase boundary. Solid/liquid/liquid/gas.
    • Reduction reaction is always written on the right.
    • ' || ' denotes the salt bridge. Eliminates liquid junction potential.
    • Metal electrodes are always the outermost components in the notation.
    • Examples: Pt| Fe²⁺/Fe³⁺, AgCl/Ag, etc.
    • Electrodes can share the same electrolyte. Example: H₂ → 2H⁺ + 2e⁻ and AgCl(s) + e⁻ → Ag + Cl⁻.

    Liquid Junction Potential

    • If two solutions of different concentrations are separated by a porous barrier, H⁺ ions will cross from higher concentration to lower, at a faster rate than Cl⁻ ions, leading to a potential difference across the barrier, also called Liquid Junction Potential.
    • The steady state potential difference is eliminated by using a salt bridge.
    • A salt bridge containing ions of similar mobility (e.g., KCl, KNO3) is used to balance charges.

    Entropy and Enthalpy

    • The thermodynamic parameters of an electrochemical cell can be calculated.
    • The electrical work done is -nFEcell , and Gibbs free energy, ΔG = H − TS.

    Energy Level View of Electron Transfer

    • Electrons in solution have discrete atomic/molecular orbitals, in metals where many atoms bond, these orbitals overlap to produce an energy band.
    • When a metal and an ion in solution interact, electrons transfer between the two. Electrons in the metal originate from the top of the conduction band.
    • Equilibrium is reached when electron energy levels on both the metal and ion side match.

    Fundamentals of Electron Transfer Reactions

    • Galvanic cells develop potential spontaneously. A half-cell is a terminal. Chemical potential drives electron flow. Electrochemical reaction rate is given as the current (I, A) or current density (i, A m⁻²).
    • Electrode area (A) in determining current density.
    • Non-spontaneous reactions are possible by applying a potential difference to an electrode, driving the reaction artificially. Examples are Faradaic Cells.

    Tafel Equations

    • The Butler-Volmer equation describes the relationship between current density and overpotential. For large overpotentials, the exponential relationship is simpler & useful
    • For oxidation: positive overpotential, oxidation reaction dominates, anodic Tafel Equation.
    • For reduction: negative overpotential, reduction reaction dominates, cathodic Tafel Equation.

    Overpotential

    • E is the equilibrium potential for the electron transfer process
    • Eapp is the applied potential
    • Overpotential is a measure of the difference between the applied potential and the equilibrium potential.

    Mass Transfer

    • Eventually, the rate of the electrochemical reaction becomes limited by the rate of diffusion of reactants to the surface from the bulk solution.
    • The maximum or 'mass transport limiting' current can be estimated.

    Example Calculations

    • Example problems involving calculation of current density, using given data and the Tafel equation will be presented for various conditions.

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    Test your knowledge on electrochemistry with this comprehensive quiz covering essential topics like electrochemical cells, Nernst Equation, and corrosion. Explore the principles of battery technology and fuel cells, including their applications and future prospects. Perfect for students looking to deepen their understanding of electrochemical processes.

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