Electrode Deposition and Batteries

Electrodeposition

  • Calculating the amount of substance deposited on an electrode surface.
  • Determined by the total time of electrode.

Calculation Steps

  1. Check the chemical equation.

  2. Determine the AEP (Amount of Electrons Passed), which is specific to one half-reaction.

    • Not for overall environment.

Example

  • Combination of reduction processes, involving nickel.

q (charge) over F (Faraday's constant) yields moles of nickel.

  • F in coulombs per mole.

\frac{q}{F} = \text{moles of nickel}

  • Moles of nickel multiplied by the molar mass of nickel gives the mass of nickel.

PPT Reaction in Sewer

  • Given mass of sewer and amperage (A).
  • Determine the time required (in seconds, minutes, or hours).
  • n \cdot F = q, where n is the number of electrons.
  • q/I = t, where I is current (amperes) and t is time (seconds).
  • 1 coulomb = 1 ampere * second.
  • Time in seconds, then divide to get minutes.

Moment Code

  • Moles of electron (n) times Faraday's constant (F) equals the charge (q).

Reverse Reaction

  • Time should be converted into seconds.

Batteries

  • Understanding the basic idea of how batteries work.
  • Distinguishing between primary and secondary batteries.
  • Batteries are galvanic cells that generate electrical energy.
  • Use selection of various cell
  • Nickel cadmium batteries are rechargeable.
  • Batteries have size limitations in small devices like cell phones, laptops, and cameras.
  • Hydrogen gas can be converted into metal hydride.

Nickel Metal Hydride Battery

  • Offers better power per volume (electric energy density) compared to nickel-cadmium batteries.
  • Understanding active reactions is crucial.
  • Distinguish primary and secondary.

Lithium Ion Batteries

  • Generate electricity/electrical charge.

Proton

  • Special type of galvanic cell.
  • Hydrogen gas loses electrons in water.
  • Reactants: Oxygen gas and hydrogen gas.
  • Oxygen gas pumped into the cathode, hydrogen gas into the anode.
  • Products: Hydroxide and water.
  • Reaction involves no other chemicals besides water.

Metal Refining

  • Refining metals to reduce the outside layer.
  • Copper sheets: Pure copper on both sides.
  • Pure copper as anode and cathode.
  • Electrolyte: Copper sulfate.

Corrosion

  • Application involving iron.
  • Iron can be coated by iron oxide when exposed to oxygen.

Handle Protection

  • Protecting iron by separating it from other metals or applying protective measures.
  • Use panel

Review

  • Applications reviewed from the previous section (2019).