An electrochemist investigates the electrolysis of an aqueous silver nitrate solution, AgNO3\text{AgNO}_3AgNO3, to silver-plate a key. During this process, silver is deposited onto the cathode (negative electrode). The table below shows the mass of silver deposited over time.
| Time (minutes) | Mass of silver (g) |
|---|---|
| 0 | 0.00 |
| 15 | 0.27 |
| 30 | 0.54 |
| 45 | 0.81 |
| 60 | 1.08 |
| 75 | 1.35 |
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.