The reaction between nitrogen monoxide and hydrogen at high temperatures is represented by the equation below:
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)Under specific conditions in a combustion simulation, the rate constant, kkk, for this reaction is determined to have the units dm9 mol−3 s−1\text{dm}^9\text{ mol}^{-3}\text{ s}^{-1}dm9 mol−3 s−1.
What is the overall order of this reaction?
2
3
4
5
