https://padlet.com/m2194739/chemy_f5_electrolytic_cell Chapter 1.4 en-us 2021-05-21 13:15:54 UTC 2023-05-03 07:36:28 UTC hello@padlet.com m2194739 https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1547583628 Electrolysis is a process whereby compounds in the molten state or an aqueous solution decompose into their constituent elements by passing electricity through them.

• Electrolytes are substances that can conduct electricity in either the molten state or aqueous solution and undergo chemical changes.
• Non-electrolytes are substances that cannot conduct electricity in all states.

]]> 2021-05-21 13:17:32 UTC https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1547583628 m2194739 https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1547915544 Classifications ]]> 2021-05-21 14:40:02 UTC https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1547915544 m2194739 https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1547934290 Conductors :-
# substance that conduct electricity in solid or molten state, but do not undergo chemical changes
# conduct electricity without undergoing decomposition
# can conduct electricity due to the presence of electrons that move freely
# electrical conductivity decreases as temperature increases
# exp: metals, graphite

Electrolyte :-
# substance that conduct electricity in molten state or aqueous solution, and undergo chemical changes
# conduct electricity and undergo decomposition into their constituent elements
# can conduct electricity due to the presence of ions that move freely
# electrical conductivity increases as temperature increases.
# exp: ionic compounds, acids, alkalis.]]> 2021-05-21 14:44:41 UTC https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1547934290 m2194739 https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1548031011 2021-05-21 15:07:45 UTC https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1548031011 m2194739 https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1548061844

E0 Value

Concentration of solution

Type of electrode used
- anode
- cathode 

• Water also takes part in the electrolysis process.
• The equation for water dissociation is as follows: H2O(l) ⇌ H+(aq) + OH−(aq)
• During electrolysis, cations and hydrogen ions, H+ move to the cathode, while anions and hydroxide ions, OH− move to the anode.

]]> 2021-05-21 15:15:27 UTC https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1548061844 m2194739 https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1548107927 2021-05-21 15:26:13 UTC https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1548107927 m2194739 https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1548159158 Similarities
S1- Electrodes are dipped into the electrolyte
S2- Oxidation reactions at the anodes
S3- Reduction reactions at the cathodes
S4- Electrons flow from the anodes to the cathodes through the connecting wires

Differences

Voltaic cell:-
D1- Chemical energy to electrical energy
D2- Pairs of metals are of different types
D3- Negative terminal is anode and positive terminal is cathode
D4- Blue colour of copper(II) sulphate, CuSO4
solution becomes paler

Electrolytic cell:-
D1- Pairs of metals are the same type
D2- Electrical energy to chemical energy
D3- Blue colour of copper(II) sulphate, CuSO4 solution does not change 
D4- Anode is connected to the positive terminal of the battery and cathode is connected to the battery’s negative terminal

]]> 2021-05-21 15:38:19 UTC https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1548159158 m2194739 https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1548171226 2021-05-21 15:41:05 UTC https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1548171226 m2194739 https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1548200416 Electroplating of metals through electrolysis is done by:-
# making the object being electroplated as the cathode, the electroplating metal as the anode, and an aqueous solution containing the ions of the electroplating metal as the electrolyte]]> 2021-05-21 15:47:42 UTC https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1548200416 m2194739 https://padlet.com/m2194739/chemy_f5_electrolytic_cell/wish/1548217169 # Copper is an important mineral and element in our daily life. It is an important industrial metal due to its ductility, malleability, electrical conductivity and resistance towards corrosion.

# Copper used in electrical wiring must have a 99.99% purity. The purity of copper extracted by the process of melting is about 99.5%. Even a slight difference in copper purity will negatively impact its conductivity. To determine whether a copper metal is pure, one must conduct the purification of metals through electrolysis.

# The purification of copper by electrolysis is carried out with a piece of pure, thin copper as the cathode; impure copper as the anode; and an aqueous salt solution of copper, such as copper(II) nitrate, Cu(NO3)2 as electrolyte.

# Impure copper anode ionises to form copper(II) ions, Cu2+. Copper dissolves to become copper(II) ions, Cu2+ and impurities accumulate below the impure copper anode. The anode becomes thinner.
Cu(s) → Cu2+(aq) + 2e−

# At the pure copper cathode, copper(II) ions, Cu2+ are discharged to form copper atoms, Cu. Solid copper is deposited and the copper cathode becomes thicker.
Cu2+(aq) + 2e− → Cu(s)

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