Which of the following rate laws suggests that the reaction probably occurs in a single step?
why is this problem cant be answer a since it has order of 1
a)(CH3)3CBr + OH- →(CH3)3COH + Br- rate = k[(CH3)3CBr]
b)NO(g) + O2(g) → NO2(g) + O(g) rate = k[NO][O2]
c)H2O2 + 3 I- + 2 H+→ I3- +2H2O
rate= kl[H2O2][I-]+K2[H2O2][I-][H+]
d)H2(g) + Br2(g) → 2 HBr(g)
rate = k[H2][Br2]1/2
To determine which of the rate laws suggests that the reaction probably occurs in a single step, we should look for the rate law that only includes the reactants and no other factors. In other words, we are looking for a rate law that is solely dependent on the concentrations of the reactants and does not contain the concentration of any intermediates or catalysts.
Let's analyze each of the rate laws given:
a) (CH3)3CBr + OH- → (CH3)3COH + Br- rate = k[(CH3)3CBr]
This rate law only includes the concentration of (CH3)3CBr, the reactant. It does not contain any intermediates or catalysts. Therefore, this suggests that the reaction occurs in a single step.
b) NO(g) + O2(g) → NO2(g) + O(g) rate = k[NO][O2]
This rate law includes the concentrations of both NO and O2, indicating that this reaction may involve multiple steps.
c) H2O2 + 3 I- + 2 H+ → I3- + 2 H2O
rate= k1[H2O2][I-] + k2[H2O2][I-][H+]
This rate law includes the concentrations of H2O2, I-, and H+. The presence of multiple terms suggests that this reaction occurs through multiple steps.
d) H2(g) + Br2(g) → 2 HBr(g)
rate = k[H2][Br2]^1/2
This rate law includes the concentration of H2 and the square root of Br2, indicating that this reaction is not likely to occur in a single step.
Based on the analysis, the rate law that suggests that the reaction probably occurs in a single step is option a) (CH3)3CBr + OH- → (CH3)3COH + Br- with a rate law of rate = k[(CH3)3CBr].