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
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].
This is because a rate law with a single reactant concentration term ([Reactant]) indicates that the reaction proceeds in a single step. In this case, the rate law only includes the concentration of (CH3)3CBr, suggesting that the reaction occurs in a single step.
Option b) has two reactant concentration terms ([NO] and [O2]), which suggests that the reaction occurs through more than one step.
Option c) has three reactant concentration terms ([H2O2], [I-], and [H+]), indicating that the reaction occurs through multiple steps.
Option d) has two reactant concentration terms, but one of them is raised to the power of 1/2 ([H2][Br2]1/2), suggesting that the reaction occurs through multiple steps.
To determine which rate law suggests that the reaction probably occurs in a single step, we need to examine the orders of the reactants in each rate law. If the rate law only includes the concentrations of the reactants and the exponents of those concentrations are all 1, it suggests that the reaction is likely to occur in a single step.
Let's analyze each of the rate laws provided:
a) Rate = k[(CH3)3CBr] - This rate law has an order of 1 with respect to [(CH3)3CBr]. This means that the reaction occurs in a single step.
b) Rate = k[NO][O2] - This rate law has orders greater than 1 with respect to both [NO] and [O2]. Therefore, it suggests that the reaction occurs in multiple steps rather than a single step.
c) Rate= kl[H2O2][I-]+K2[H2O2][I-][H+] - This rate law includes multiple reactants with different exponents. It suggests that the reaction occurs in multiple steps. The included terms also indicate that there might be more than one elementary step involved.
d) Rate = k[H2][Br2]1/2 - Although this rate law contains multiple reactants, the exponent of [Br2] is 1/2. This indicates that the reaction proceeds in a fractional order with respect to [Br2], which suggests a complex reaction mechanism involving multiple steps.
Therefore, the rate law in option a) [(CH3)3CBr + OH- → (CH3)3COH + Br- rate = k[(CH3)3CBr)] suggests that the reaction probably occurs in a single step.