I really really need help with this question.... I\'m completely lost... (disreg
ID: 866659 • Letter: I
Question
I really really need help with this question....
I'm completely lost... (disregard the answer at the bottom)
Thank you guys!!!
The mechanisam for the reaction described by the equation 2N2O5(g) rightarrow 4NO2(g)+O2(g) is suggested to be N2O5(g) NO2(g)+NO3(g) NO2(g)+NO3(g) rightarrow NO2(g)+O2(g)+NO(g) NO(g)+N2O5(g) rightarrow 3NO2(g) Assuming that [No3] is governed by steady -state conditions, derive the rate law for the production of O2(g) and enter it in the space below rate of reaction = Delta[O2]/Deltat = K[N2O5]Explanation / Answer
The reaction and rate law for the gas-phase decomposition of dinitrogen pentaoxide are
2N2O5(g) ? 4NO2(g) + O2(g)
rate = k[N2O5]
Which of the following are valid mechanisms for the reaction?
1.
N2O5 ? NO3(g) + NO2(g) [fast]
NO2(g) + N2O5(g) ? 3NO2(g) + O(g) [slow]
NO3(g) + O(g) ? NO2(g) + O2(g) [fast]
2.
one step collision
3.
2[N2O5(g) ? NO3(g) + NO2(g)] [slow]
2[NO3(g) ? NO2(g) + O(g)] [fast]
2O(g) ? O2(g) [fast]
4.
2N2O5(g) ? N4O10(g) [slow]
N4O10(g) ? 4NO2(g) + O2(g) [fast]
5.
2N2O5(g) ? 2NO2(g) + N2O3(g) + 3O(g) [fast]
N2O3(g) + O(g) ? 2NO2(g) [slow]
2O(g) ? O2(g) [fast]
These are proposed mechanisms.
the rate says there is a order of one in respect of N2O5
and this will be the rate determining step.
Only those with slow N2O5 are selected. 3 and 4
as possibilities.
However the overall rate says "One step" which tends to indicate 4.
Under kinetic theory this invovles one collision which then separates. One collision is a overall rate order of one.
3. has two collisions. Overall rate order of 2.