Electrolysis Flashcards
why do covalent compounds not conduct electricity?
They have no delocalized electrons that can carry charge
why can ionic compounds conduct electricity when molten or in an aqueous solution
because then there are delocalized electrons that can carry charge
positive ions are called what
cations
negative ions are called what
anions
describe the experiment to investigate the electrolysis of lead(II) bromide
- Power supply at 12V, separate rods and lower into lead bromide powder
- Roaring Bunsen flame to melt powder in crucible
- Adjust current to 1.5A
- Brown colour of bromine seen, moist universal indicator paper held in vapour, it goes to red/slightly bleached
- Maintain for 15 minutes, then pour molten lead bromide into second crucible, keeping molten lead in the first
- Cooled lead can be marked with a fingernail
In the electrolysis of sodium carbonate solution, what are the products formed at each electrode?
Cathode - Hydrogen
Anode - Oxygen
Why do you think the anode gets smaller over time in the electrolysis of potassium nitrate?
Oxygen reacts with the carbon electrode forming CO2
- Write half-equations for the reactions occurring at each electrode in the electrolysis of potassium chloride solution. Label which is oxidation and which is reduction.
2H+ + 2e- –> H2 - reduction
2Cl- –> Cl2 + 2e- - oxidation
Write the half-equations for electrolysis of sodium chloride solution
2Cl- –> Cl2 + 2e-
2H+ + 2e- –> H2
Describe the experiment of the electrolysis of sodium chloride
- Two carbon electrodes connected to a battery in two upside down glass tubes surrounded by concentration sodium chloride solution within a beaker with a rubber bung
- add 4 drops of universal indicator and stir
- once some gas collected stop/switch off
- use damp blue litmus to test gas at anode
describe the experiment of the electrolysis of dilute sulphuric acid
- setup hoffman voltameter with power supply and sulphuric acid
- glowing splint to test gas at anode
- lit splint to test the gas at cathode
what are the five parts of the hoffman voltameter
bulb, stopcock, central tube, anode, cathode
describe the experiment of the electrolysis of copper(II) sulphate
- beaker with copper(II) sulphate solution
- two carbon (graphite) electrodes connected to 6V DC power supply
Write the ionic half equations for the electrolysis of sodium chloride
2Na+ + 2e- –> 2Na
2Cl- –> Cl2 + 2e-
Write the ionic half equations for the electrolysis of sulphuric acid
2H+ + 2e- → H2
4OH- → O2 + 2H2O + 4e-