For this problem, we have to write the rate law for this reaction in terms of -d[H2]/dt using steady-state approximation
Recall that the rate law only focuses on the reactant concentrations and has a general form of:
k = rate constant
A & B = reactants
x & y = reactant orders
The proposed mechanism for a given reaction is as follows:
Step One: 2 NO (g) N2O2 (g)
Step Two: H2(g) + N2O2(g) H2O(g) + N2O(g) Rate - determining Step
Step Three: N2O(g) + H2(g) N2(g) + H2O(g) Fast
Use the steady-state approximation on intermediates to write the rate law for this reaction in terms of . Your law should include only elementary rate constants and species that appear in the overall reaction. Show all work to support your reasoning and answer. Note: you may Not assume step one is a fast pre-equilibrium.
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Our tutors have indicated that to solve this problem you will need to apply the Reaction Mechanism concept. If you need more Reaction Mechanism practice, you can also practice Reaction Mechanism practice problems.
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Our tutors rated the difficulty ofThe proposed mechanism for a given reaction is as follows:St...as high difficulty.