Nitric oxide (NO\text{NO}NO) reacts with oxygen in the atmosphere to form nitrogen dioxide, a key step in the formation of photochemical smog. The rate equation for this termolecular-like process is:
Rate=k[NO]2[O2] \text{Rate} = k[\text{NO}]^2[\text{O}_2] Rate=k[NO]2[O2]What are the units of the rate constant, kkk, for this reaction?
mol−1 dm3 s−1\text{mol}^{-1}\text{ dm}^3\text{ s}^{-1}mol−1 dm3 s−1
mol−2 dm6 s−1\text{mol}^{-2}\text{ dm}^6\text{ s}^{-1}mol−2 dm6 s−1
mol−2 dm3 s−1\text{mol}^{-2}\text{ dm}^3\text{ s}^{-1}mol−2 dm3 s−1
mol2 dm−6 s−1\text{mol}^2\text{ dm}^{-6}\text{ s}^{-1}mol2 dm−6 s−1
