The results of an investigation into the kinetics of the reaction between NO\text{NO}NO and H2\text{H}_2H2 at a constant temperature are shown in the table below:
| Experiment | Initial [NO]/mol dm−3[\text{NO}] / \text{mol dm}^{-3}[NO]/mol dm−3 | Initial [H2]/mol dm−3[\text{H}_2] / \text{mol dm}^{-3}[H2]/mol dm−3 | Initial rate / mol dm−3 s−1\text{mol dm}^{-3}\text{ s}^{-1}mol dm−3 s−1 |
|---|---|---|---|
| 1 | 0.200 | 0.400 | 0.0320 |
| 2 | To be calculated | 0.100 | 0.0180 |
The rate equation for the reaction is:
rate=k[NO]2[H2] \text{rate} = k [\text{NO}]^2 [\text{H}_2] rate=k[NO]2[H2]What is the initial concentration of NO\text{NO}NO in experiment 2?
0.0900.0900.090
0.3000.3000.300
0.4500.4500.450
1.801.801.80
32 exam-style questions on AQA A Level Chemistry Rate equations (A-level only), covering Rate equations (A-level only) and Determination of rate equation (A-level only). Each one has a worked solution and a mark scheme showing where the marks go.