CHEM1102 Electrochemistry Equations

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247903
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CHEM1102 Electrochemistry Equations
Updated:
2013-11-20 08:01:27
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chemistry 1b electrochemistry equations
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CHEM1102 Electrochemistry Equations
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  1. Oxidation is what?
    Reduction is what?
    • Oxidation
    • Is
    • Loss of electrons
    • Reduction
    • Is
    • Gain in electrons
  2. Anode and Cathode
    polarity?, ox/red?, flow?
    • Anode    - is where oxidation occurs (vowels)
    •             - is negative
    • Cathode - is where reduction occurs (const.)
    •             - is positive
    • Electron flow: Anode ---> Cathode
  3. Standard Reduction Potential
    • ε0 
    • +ve is better at reduction (cathode)
  4. Standard Cell Potential
    E0cell =
    E0cell = ε0cathode - ε0anode
  5. Electrochemistry
    Gibb's Free Energy
    ΔG0 =
    • ΔG0 = ΣvBΔfG0
    •        = nFE0cell

    • where VB = + for prod and - for react
    • where F = 96485 Cmol-1
  6. Nernst Equation
    Ecell =
    E0cell =
    • Ecell = E0cell - (RT/nF) lnQ
    • E0cell = (RT/nF) lnK

    (cell reaction is unidirectional at +0.3V)
  7. Solubility
    For Standard Hydrogen Electrode
    εother
    (find s)
    • εother = ε0other - (RT/nF) ln (1/[solution]m)
    • (s is [solution] (mol L-1), and m is co-efficient moles of soluble ion)
  8. Electrolysis
    Q =
    • Q = ξ nF
    • Q = It
    • where ξ is extent of reaction in moles
    • I is current
  9. Evolution of Oxygen
    - reaction
    - what is standard reduction potential when it happens?
    ε =
    • O2 + 4H+ + 4e- = 2H2O
    • SRP is +ve
    • ε = ε0 - (RT/4F) ln (1/(PO2[H+]4))
  10. Evolution of Hydrogen
    - reaction
    - what is standard reduction potential when it happens?
    ε =
    • 2H+ + 2e- = H2
    • SRP is -ve
    • ε = ε0 - (RT/2F) ln (PH2/[H+]2)

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