consider the following reaction mechanism
2A+B->B+C
B+D->E+C
What is the rate law for step 2 of this reaction?
To determine the rate law for step 2 of the reaction mechanism, we need to identify the reactants involved and their respective reaction orders.
Looking at the reaction: B + D -> E + C
We can see that the reactants involved in this step are B and D. To find the reaction order for each of these reactants, we need to examine the stoichiometry of the reaction in this step.
From the reaction, we can see that the rate of the reaction is dependent on the concentration of B, which suggests that B is a reactant. Therefore, the reaction order for B is 1.
Similarly, D is also a reactant in this step. However, we don't have any information about the stoichiometry of the reaction with respect to D. Without that information, we cannot determine the specific reaction order for D.
Therefore, the rate law for step 2 of this reaction can be written as: Rate = k[B]^1[D]^x, where x is the unknown reaction order for D.