Please explain clearly and with steps if possible! thank you :) Question 6 of 25

Question

Please explain clearly and with steps if possible! thank you :)

Question 6 of 25 General Chemistr Donald McQuarrie Peter A. Rock Ethan Gallogly University Science Books presented by Sapling The mechanism for the reaction described by the equation 2N,O is suggested to be (1) N,0,(g) No,W-Nole) (3) No^)+N,O,(g Assuming that [NO3l is govermed by steady-state conditions, derive the rate law for the production of OXg) and enter it in the space below. rate of reaction O Previous Give Up & View Solution Check Answer 0 Next Exit Hin

Explanation / Answer

In the reaction, [NO] and [NO3] are intermediates

Applying steady state approximation,

rate of production of intermediate = rate of consumption of intermediate

For [NO3],

k1[N2O5] = k-1[NO2][NO3] + k2[NO3][NO2]

[NO3] = k1[N2O5]/(k-1 + k2)[NO2] ------ (1)

Now we can write,

d[O2]/dt = k2[NO2][NO3] -------- (2)

Feed (1) in (2),

d[O2]/dt = k2[NO2].k1[N2O5]/(k-1 + k2)[NO2]

              = k1k1[N2O5]/(K-1 + k2)

with, k = k1.k2.(k-1 + k2)

we get,

rate law for O2,

d[O2]/dt = k[N2O5]

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