Exp. 2 Faraday's Law of Electrolysis

• Electrolysis


  Non-spontaneous oxidation-reduction reactions occurred by electric current through electrolyte solution
• Electrolytic cell


  Cell that perform electrolysis
• Galvanic cell


  cell that converts the chemical energy of spontaneous redox reactions into electrical energy
• Oxidation, Anode, positive

  A) M

  B) M^v+

  C) ve-

  
• Reduction, Cathode, minus

  A) 2H+

  B) (aq)

  C) +2e-

  D) H2(g)

  
• To produce balanced oxidation-reduction reaction, number of electrons lost by "oxidation half-reduction equation = number gained by reduction half-reaction"
• Mass of metal lost at the anode depends upon both its molar mass
• If v=2, overall reaction equation

  A) M(s)

  B) +

  C) 2H+(aq)

  D) M^2+(aq)

  E) +

  F) H2(g)

  
• if v=1, we must double the equation

  A) 2M(s)

  B) +

  C) 2H+(aq)

  D) 2M+(aq)

  E) +

  F) H2(g)

  
• Relationship between mass of metal lost

  A) M

  B) v

  C) mass of metal lost per mole of

  D) electrons used in the electrolysis

  
• Faraday's law of electrolysis

  n= number of moles of electrons transferred

  m=mass of metal lost

  v=electrons used in electrolysis

  A) M

  B) mv

  C) n

  
• Water pressure in burette

  A) p

  B) g

  C) h

  D) density of liquid = 1000kg/m^3

  E) gravity = 9.8m/s^2

  F) height of liquid

  
• Moles of H2 gas

  A) P

  B) P=Pressure (Pa)

  C) V

  D) V=volume (m^3)

  E) n

  F) n=number of moles

  G) R

  H) R=Gast consant (JK mole)

  I) T

  J) T=Temperature (K)

  
• Faraday's Law of Electrolysis deals with the relationship between the quantity of electricity passed and the equivalent weight of the substance deposited at the electrodes.
• $CH_3COOH$Weak acid

  $Na_4SO_4$Salt