fast no+no-->n2o2,
slow n2o2+h2-->n2o+h20,
fast n2o+h2-->n2+h2o
1)What is the intermediates in the rxn
2)Write the rate law for this process
To determine the intermediates in this reaction and write the rate law, we need to examine the overall reaction as well as the individual steps.
The overall reaction is:
2 NO + 2 H2 -> N2 + 2 H2O
Based on the given steps and the overall reaction, we can identify the intermediates.
1) To identify the intermediates:
The species that are formed in one step and consumed in a subsequent step are the intermediates. In this case, the intermediates are N2O and H2O.
From the first step:
fast no + no -> n2o2
The intermediate formed here is N2O2.
From the second step:
slow n2o2 + h2 -> n2o + h2o
The intermediate formed here is H2O.
2) To write the rate law:
The rate law represents the relationship between the rate of the reaction and the concentrations of the reactants.
From the given steps, let's determine the rate-determining step:
The slowest step in a reaction usually determines the overall rate of the reaction. In this case, it is the second step:
slow n2o2 + h2 -> n2o + h2o
The rate law for the rate-determining step can be written as follows:
rate = k * [N2O2]^a * [H2]^b
Since the coefficients in the rate-determining step are 1 for N2O2 and 1 for H2, the exponents "a" and "b" would both be 1.
Therefore, the rate law for this process is:
rate = k * [N2O2] * [H2]