A reversible reaction between three dissolved substances, J, K and L, takes place in a closed reaction cell. The conditions are kept constant.
J(aq)⇌K(aq)+L(aq)\mathrm{J(aq) \rightleftharpoons K(aq) + L(aq)}J(aq)⇌K(aq)+L(aq)
The table shows the measured rates of the forward and reverse reactions.
| Time (min) | Rate of forward reaction (mmol/min) | Rate of reverse reaction (mmol/min) |
|---|---|---|
| 0 | 1.20 | 0.00 |
| 2 | 0.95 | 0.25 |
| 4 | 0.78 | 0.42 |
| 6 | 0.66 | 0.54 |
| 8 | 0.60 | 0.60 |
Which time in the table first shows that the mixture has reached dynamic equilibrium?
Explain your answer, including why the equilibrium is described as dynamic, and predict what happens to the amounts of J, K and L after this time.
124 exam-style questions on OCR GCSE Chemistry 5.3 Equilibria, covering 5.3.1 Reversible reactions and dynamic equilibrium and 5.3.2 Changing the position of equilibrium. Each one has a worked solution and a mark scheme showing where the marks go.