Electrochem II Flashcards
What is electrolytic cell?
The process in which electrical energy is used to bring about non-spontaneous redox reaction
Where does electrolysis take place?
- in electrolytic cell which consists of a pair of electrodes to carry an electric current into and out of the cell
- with an electrolyte, a compound in aqueous or molten state which conducts an electric current due to presence of mobile ions
Is anode positive or negative in an electrolytic cell?
Positive (rmb: PANIC: Positive Anode, Negative Is Cathode)
What does anode in an electrolytic cell attract?
Anions (rmb: Anode attracts anions)
What reaction takes place at the anode for an electrolytic cell?
Anions are oxidised because they lose electrodes (rmb: an-ox)
Is cathode positive or negative in an electrolytic cell?
Negative (rmb: PANIC: Positive Anode, Negative Is Cathode)
What does cathode attract in an electrolytic cell?
Cations (rmb: cathode attracts cations)
What reaction takes place at the cathode for an electrolytic cell?
Cations are reduced because they gain electrons (rmb: red - cat)
What is the flow of electrons and why?
From cathode (-) anode (+)
Electrons move from lower potential to higher potential (think physics circuit, opposite of current)
What are the factors affecting the identity of substances liberated?
- State of electrolyte (molten or aqueous)
- Position of species in the redox series
- Concentration of species in the electrolyte
- Nature of electrode
How does the state of electrolyte affect the identity of substance liberated?
- molten electrolyte: only consider cations at cathode and anions at anode
- aqueous electrolyte: need consider water at both cathode and anode (water is present at large quantities)
What is the equation for the reduction of water?
2H2O (l) + 2e- –> H2 (g) + 2OH- (aq)
What is the equation of the oxidation of water?
2H2O (l) –> 4H+ (aq) + O2 (g) + 4e-
How does the position of species in the redox series affect the identity of substance liberated?
- species with more positive E naught value is more readily reduced
- species with less positive E naught value is more readily oxidised
Since water can auto-ionise, why does reduction of H+ and oxidation of OH- not occur?
[H+] and [OH-] are too low compared to concentration of H2O and hence not considered