The reaction between nitrogen monoxide and oxygen is represented by the following rate equation:
rate=k[NO]2[O2] \text{rate} = k[\text{NO}]^2[\text{O}_2] rate=k[NO]2[O2]Which statement is correct?
The rate of reaction increases by a factor of 18 if the concentration of NO\text{NO}NO is tripled and the concentration of O2\text{O}_2O2 is doubled.
The rate constant has units of mol−1dm3s−1\text{mol}^{-1} \text{dm}^3 \text{s}^{-1}mol−1dm3s−1.
The rate of reaction is multiplied by 4 if the concentration of NO\text{NO}NO is doubled and the concentration of O2\text{O}_2O2 is halved.
The rate constant increases when the concentration of NO\text{NO}NO is increased.
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.