Problem: 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 StepStep Three: N2O(g) + H2(g)    N2(g) + H2O(g)    FastUse 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.

FREE Expert Solution

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:

rate law=kAxBy

k = rate constant
A & B = reactants
x & y = reactant orders

  • A steady-state approach makes use of the assumption that the rate of production of an intermediate is equal to the rate of its consumption.
  • We will be starting this with:

Rate law = -d[H2]dt= k2[H2][N2O2] (1)

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Problem Details

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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