An engineer tests two reaction cells. In each cell, gas X changes reversibly into gas Y.
X(g)⇌Y(g)\text{X(g)} \rightleftharpoons \text{Y(g)}X(g)⇌Y(g)
Each cell initially contains 1.00 mol of X and no Y. The temperature remains constant. If no gas escapes, the total amount of X and Y remains 1.00 mol.
One cell has a damaged wall that allows gas to escape.
| Time in minutes | Amount of X in cell A in mol | Amount of Y in cell A in mol | Amount of X in cell B in mol | Amount of Y in cell B in mol |
|---|---|---|---|---|
| 5 | 0.62 | 0.38 | 0.56 | 0.34 |
| 10 | 0.48 | 0.52 | 0.39 | 0.42 |
| 15 | 0.40 | 0.60 | 0.29 | 0.44 |
| 20 | 0.40 | 0.60 | 0.26 | 0.40 |
Use the data to explain which cell has reached dynamic equilibrium by 20 minutes and which cell has a damaged wall.
109 exam-style questions on AQA GCSE Chemistry 6.2 Reversible reactions and dynamic equilibrium, covering 6.2.1 Reversible reactions, 6.2.2 Energy changes and reversible reactions, 6.2.3 Equilibrium, 6.2.4 The effect of changing conditions on equilibrium, 6.2.5 The effect of changing concentration, 6.2.6 The effect of temperature changes on equilibrium, and 6.2.7 The effect of pressure changes on equilibrium. Each one has a worked solution and a mark scheme showing where the marks go.