Redox...

Front 1

Consider how current is conducted in an electrolytic cell. Which statement is correct?
A. Electrons move through the electrolyte and the external circuit.
B. Ions move through the electrolyte and the external circuit.
C. Electrons move through the external circuit and ions move through the electrolyte.
D. Electrons move through the electrolyte and ions move through the external circuit.

Back 1

C

Front 2

Electrolysis has made it possible to obtain reactive metals such as aluminium from their ores, which has resulted in significant developments in engineering and technology. State one reason why aluminium is preferred to iron in many uses.

Back 2

Al does not corrode/rust / Al is less dense/better conductor/more malleable;

Front 3

Outline two differences between an electrolytic cell and a voltaic cell.

Back 3

electrolytic cell converts electrical energy to chemical energy and voltaiccell converts chemical energy to electrical energy / electrolytic cell uses
electricity to carry out a (redox) chemical reaction and voltaic cell uses a
(redox) chemical reaction to produce electricity / electrolytic cell requires
a power supply and voltaic cell does not;
electrolytic cell involves a non-spontaneous (redox) reaction and voltaic
cell involves a spontaneous (redox) reaction;
in an electrolytic cell, cathode is negative and anode is positive and vice-versa
for a voltaic cell / electrolytic cell, anode is positive and voltaic cell,
anode is negative / electrolytic cell, cathode is negative and voltaic
cell, cathode is positive;
voltaic cell has two separate solutions and electrolytic cell has one
solution / voltaic cell has salt bridge and electrolytic cell has no salt bridge;
electrolytic cell, oxidation occurs at the positive electrode/anode and voltaiccell, oxidation occurs at the negative

Front 4

For the Sn(SO4)2 cell, suggest two factors, other than time and current, that would affect the amount of metal deposited during electroplating.

Back 4

temperature of solution;
[Sn4+];
surface area/size of electrode;
material of electrodes;

Front 5

Define standard electrode potential.

Back 5

the potential difference/voltage obtained when a half-cell is
connected to a standard hydrogen electrode;
under standard conditions / 1.00 mol dm–3 solutions, 298 K;