The gas-phase reaction between nitrogen monoxide and hydrogen is represented by the following equation:
2NO(g)+2H2(g)→N2(g)+2H2O(g) 2\text{NO}(\text{g}) + 2\text{H}_2(\text{g}) \rightarrow \text{N}_2(\text{g}) + 2\text{H}_2\text{O}(\text{g}) 2NO(g)+2H2(g)→N2(g)+2H2O(g)The experimentally determined rate equation for this reaction is:
Rate=k[NO]2[H2] \text{Rate} = k[\text{NO}]^2[\text{H}_2] Rate=k[NO]2[H2]What are the units of the rate constant, kkk?
mol2 dm−6 s−1\text{mol}^{2}\text{ dm}^{-6}\text{ s}^{-1}mol2 dm−6 s−1
mol−2 dm6 s−1\text{mol}^{-2}\text{ dm}^6\text{ s}^{-1}mol−2 dm6 s−1
mol−2 dm6 s\text{mol}^{-2}\text{ dm}^6\text{ s}mol−2 dm6 s
mol−1 dm3 s−1\text{mol}^{-1}\text{ dm}^3\text{ s}^{-1}mol−1 dm3 s−1
