The decomposition of nitramide. o2nnh2. in water has the following chemical equation and rate law.

The decomposition of nitramide, O2NNH2, in water has the following chemical equation and rate law. O2NNH2 (aq) yields N2O (g) + H2O (l) rate= [O2NNH2]/[H]
A proposed mechanism for this reaction is.
k1 (1) O2NNH2 (aq) equilibrium O2NNH (aq) + H (aq) (fast equilibrium) k-1


k2 (2) O2NNH (aq) yields N2O (g) + OH (aq) (slow)

k3 (3) H (aq) + OH yields H2O (l) (fast)

What is the relationship between the observed value of k and the rate constants for the individual steps of the mechanism?

k=__________

Also which symbols go into the numerator or demoniator k-1, k3, k2, k1

Answer

General guidance

Concepts and reason
oThe rate constant of the reaction at a given temperature is defined as the rate of the reaction when the molar concentration of each of the reactants is unity. oThe rate of the reaction depends on the reactant concentration. oThe rate of a reaction is proportional to some power of the molar concentration of each of the reactants. oThe rate constant can be determined by using the rate law.

Fundamentals

Rate of the reaction in terms of concentration of the reactants that determine the rate of the reaction is called the rate law or rate equation. Rate law for a general reaction is cC+dD—>product rate=k[A] [B],
Where k is called the rate constant If the reaction proceeds through more than one step, then the overall rate of the reaction determined step is the slow step.

Step-by-step

Step 1 of 3

Consider the mechanism of the given reaction and write the rate law. Step 1. 0,NNH, (aq)<*>0,NNH(aq)+H(aq)
rate=k, [0,NNH,]
rate=k, [0,NNH][H]
Here,
k, [0,NNH,]=k, [0,NNH][H] Step 2. O,NNH(aq) k>N,0(g)+OH(aq)
rate=k, [O,NNH] This is the overall rate determined step Step 3. H(aq) +OHks »H,0(1)
rate=kz [H](OH) Rate law of the decomposition reaction is rate=k[, NNH,
H

The reaction equation is given and the rate expression for each of the reactant species is also given. Consider this given reaction and write the rate law. At the equilibrium, the rate of formation of is equal to the rate of decomposition of in step 2.

Step 2 of 3

Overall rate of the reaction is rate=k, [0,NNH)....(2) Consider the rate of the step 1 k[O,NNH,]=k., [0,NNH][H]
TO Nnul_k, [0,NNH,]
(0,NNH] =– , [H] Substitute the value of O,NNH in equation (2) rate=k,x [2NNH,
I k,[H]
rate = k;*k, x [0,NNH,]
k
[H] Compare the equation (1) and (3) and find the relationship rate=k O2NNH, 1
......... (1)
k,xk, [0,NNH,]
rate=-*. *[H]
(3)

Overall rate of the reaction is determined by the step 2 because it is the slow step among the other steps. Write the overall rate of the reaction, then compare the overall rate of the reaction and give rate of the reaction and find the relationship between the observed value of and the rate constants for the individual steps of the mechanism.

Step 3 of 3

Consider the equation of found in step 2. k=k,xk Numerator is k, andk Denominator is

The relationship between the observed value of and the rate constants for the individual steps of the mechanism is k=k,xk Numerator is k, andk Denominator is


The fraction contains two parts, top and bottom parts. The numerator is the top of the fraction and the denominator is the bottom of the fraction. So in fraction, k, andk are the numerators and is the denominator.

Answer

The relationship between the observed value of and the rate constants for the individual steps of the mechanism is k=k,xk Numerator is k, andk Denominator is

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