An electroplating cell containing aqueous silver nitrate, AgNO3(aq)\text{AgNO}_3\text{(aq)}AgNO3(aq), was operated at a constant electric current. During this electrolysis process, silver is deposited at the cathode (negative electrode). The table below records the mass of silver deposited over time:
| Time (minutes) | Mass of silver (g) |
|---|---|
| 0 | 0.00 |
| 15 | 0.36 |
| 30 | 0.72 |
| 45 | 1.08 |
| 60 | 1.44 |
| 75 | 1.80 |
Assuming the rate of deposition of silver remains constant, determine the mass of silver that would be produced after 50 minutes.
12 exam-style questions on AQA GCSE Chemistry 4.3 Electrolysis, covering 4.3.1 The process of electrolysis, 4.3.2 Electrolysis of molten ionic compounds, 4.3.3 Using electrolysis to extract metals, 4.3.4 Electrolysis of aqueous solutions, and 4.3.5 Representation of reactions at electrodes as half equations (HT only). Each one has a worked solution and a mark scheme showing where the marks go.