11 Question point) Q See page 646 Nitric oxide reacts rapidly with unstable nitr

Question

11 Question point) Q See page 646 Nitric oxide reacts rapidly with unstable nitrogen trioxide (NO,) to form NO, NO(g) + NO3(g) 2NO2(g) Calculate the numeric value of the rate constant for the above reaction from the data in the table below Initial Reaction Rates for the Formation of NO, by the Reaction of NO with NO, at 298 K Experiment¡Nolo(MNO!e(M) Initial Reaction Rate(MS) 20.0× 10-1 2.00+10+ | 4,00 0 8,00 10 1.60-10 4,00K 10-1 2.00× 10 13 400. 10-14.00x10-1 1st attempt ht See Periodic Table See Hlint The rate constant, k, is

Explanation / Answer

see experiment 1 and 2:

[NO] doubles

[NO3] is constant

rate doubles

so, order of NO is 1

see experiment 2 and 3:

[NO] is constant

[NO3] doubles

rate becomes 4 times

so, order of NO3 is 1

overall order = 1 + 1 = 2

Rate law is:

rate = k*[NO]*[NO3]

Put values from 1st row of table in rate law

rate = k*[NO]*[NO3]

4*10^4 = k*0.002*0.002

k = 1.0*10^10 M-1.s-1

Answer: 1.0*10^10 M-1.s-1

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