Which of the following rate laws suggests that the reaction probably occurs in a single step?
NO(g) + O2(g) → NO2(g) + O(g) rate = k[NO][O2]
H2O2 + 3 I- + 2 H+→ I3- + 2 H2O rate= kl[H2O2][I-]+K2[H2O2][I-][H+]
H2(g) + Br2(g) → 2 HBr(g) rate = k[H2][Br2]1/2
(CH3)3CBr + OH- →(CH3)3COH + Br- rate = k[(CH3)3CBr]
The rate law that suggests that the reaction probably occurs in a single step is the rate law given by:
H2(g) + Br2(g) → 2 HBr(g) rate = k[H2][Br2]1/2
In a single-step reaction, the rate law is determined solely by the reactants' concentrations, with each reactant raised to a particular power. In this case, both H2 and Br2 appear in the rate law, indicating that the reaction occurs in a single step.
To determine this, you can look at the reaction equation and the rate law equation. If the rate law equation includes all the reactants (with each reactant raised to a power), it suggests that the reaction is happening in a single step.