Use the References to access important values if needed for this question. The f

Question

Use the References to access important values if needed for this question. The following initial rate data are for the oxidation of nitrogen monoxide by oxygen at 25 °C [NO]o, M 78x10-3 7.56x10-3 3.78x10-3 7.56x10-3 xperment [02]o, M 78x10-3 3.78x10-3 7.56x10-3 7.56x10-3 al Rate, M s-1 4.69x10-4 1.88x10-3 9.38x10-4 75x10-3 Complete the rate law for this reaction in the box below. Use the form k[A]B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or Rate- From these data, the rate constant is M25-1 Submit Answer Retry Entire Group 3 more group attempts remaining Pre Next

Explanation / Answer

a)

see experiment 1 and 2:

[NO] doubles

[O2] is constant

rate becomes 4 times

so, order of NO is 2

see experiment 1 and 3:

[NO] is constant

[O2] doubles

rate doubles

so, order of O2 is 1

overall order = 2 + 1 = 3

Rate law is:

rate = k*[NO]^2*[O2]

b)

rate = k*[NO]^2*[O2]

Put values from 1st row of table in rate law

rate = k*[NO]^2*[O2]

4.69*10^-4 = k*0.00378^2*0.00378^1

k = 8684 M-2.s-1

Answer: 8684 M-2.s-1

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