Electrochemical Reactions

Question 1

Galvanic Cell

Answer 1

Cell in which chemical energy is converted into electrical energy. It has self sustaining electrode reactions

Question 2

Electrolytic Cell

Answer 2

Cell which converts electrical energy into chemical energy

Question 3

Reduction

Answer 3

Gain in electrons resulting in the gain in oxidation number of a cell. (Occurs at the cathode)

Question 4

Oxidation

Answer 4

Loss in electrons resulting in the increase in oxidation number. (Occurs at the Anode)

Question 5

Oxidising Agent

Answer 5

Substance which is reduced and gains electrons.

Question 6

Reducing Agent

Answer 6

Substance that is oxidised and loses electrons

Question 7

Anode

Answer 7

Electrode where oxidation takes place

Question 8

Cathode

Answer 8

Electrode where reduction takes place

Question 9

Electrolyte

Answer 9

Solution that conducts electricity through the movement of ions

Question 10

Electrolysis

Answer 10

Chemical process in which electrical energy is converted to chemical energy
OR
Use of electrical energy to produce a chemical change

Question 11

Name the Standard Conditions

Answer 11

Electrolyte Concentration: 1 mol.dm^-3
Temperature: 298 K (25°C)
Pressure (only relevant for gases): 1 atmosphere

Question 12

Functions of the salt bridge in a Galvanic Cell?

Answer 12

1. Completes the circuit

2. Provides a path for ion exchange to conserve electrical neutrality

Question 13

Standard Hydrogen Electrode

Answer 13

Half-cell consisting of Hydrogen gas which attaches to a platinum electrode in 1,00 mol.dm^-3 H^+ (acidic) solution.