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 the reaction, we need to look for species that are formed in one step and consumed in another. In this case, the reaction mechanism consists of three steps:
1) Fast reaction: no + no → n2o2
2) Slow reaction: n2o2 + h2 → n2o + h2o
3) Fast reaction: n2o + h2 → n2 + h2o
1) From the reaction mechanism, we can see that the intermediate species is n2o (nitrogen dioxide). It is formed in the second step and consumed in the third step.
2) The rate law is an expression that relates the rate of a chemical reaction to the concentrations of reactants. To determine the rate law for this process, we need to examine the slowest step, which is the rate-determining step. In this case, it is the second step:
Rate = k[n2o2][h2]
The rate law for the overall reaction is determined by the slow step, so the rate law is dependent on the concentrations of n2o2 and h2 raised to their respective stoichiometric coefficients. The symbol "k" represents the rate constant for the reaction.