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Electrochemistry - Coggle Diagram

- - - - Oxidizing agent stronger than reducing agent
      - Cell potential is positive
  - - - Reducing agent stronger than reducing agent
      - Requires external energy to take place
      - Cell potential is negative
    - - When chloride ions and water are only RAs, chloride ions are strongest RA. Results in chloride gas at anode instead of oxygen
  - - - Anode (where oxidation occurs)
      - Cathode (where reduction occurs)
      - Salt bridge (allows movement of ions between electrodes)
        
        Spectator ions
      - External pathway for electrons to flow
    - - Electrical potential difference (voltage) difference in energy per unit of charge between two points in circuit
        
        Calculated with standard conditions (25C, 1.0 atm, 1.0mol/L)
        
        Potentials relative to hydrogen half-cell (0.00V)
        
        Ecell = Ecathode - Eanode
        
        If potential greater than 0, spontaneous, if less than 0, nonspontaneous
    - - Parts of calculation
        
        Current (I) measured in amperes (A)
        
        Charge (Q) measured in coulombs (C)
        
        Time (t) measured in seconds (S)
        
        Faraday's Constant (F) = 95,500 C/mol e-
      - Faraday's Law of Electrolysis
        
        ne = (Q/F) = ((I x t)/F)
- - - - Reducing Agent (element that is oxidized in transfer of electrons)
    - - Oxidizing Agent (element that is reduced in transfer of electrons)
    - - Spontaneous (Potential less than zero, OA higher than RA on table of electrodes)
        
        Irreversible
      - Nonspontaneous (Potential greater than zero, RA higher than OA on table of electrodes)
        
        Reaction must have catalyst/energy added to occur
  - - - Use oxidation numbers to find charges and balance electrons
    - - Acidic
        
        Must be balanced using H2O to balance O2 and H+ to balance H molecules
      - Basic
        
        Must be balanced using H2O to balance O2, H+ to balance H, and OH- to neutralize
- - - - Find mole ration of known titrant moles (found by multiplying average volume used in titration by concentration) to moles of analyte
        
        Use mole ratio to find moles of sample, divide by volume of sample to find concentration