A reaction is performed to study the oxidation of nitrogen monoxide by oxygen at
ID: 489353 • Letter: A
Question
A reaction is performed to study the oxidation of nitrogen monoxide by oxygen at 25 °C:
The following reaction rate data was obtained in four separate experiments.
What is the rate law for the reaction and what is the numerical value of k?
Complete the rate law in the box below.
Remember that an exponent of '1' is not shown and concentrations taken to the zero power do not appear.
k =
M-2s-1
Experiment [NO]0, M [O2]0, M Initial Rate, Ms-1 1 5.70×10-3 3.80×10-3 1.05×10-3 2 1.14×10-2 3.80×10-3 4.22×10-3 3 5.70×10-3 7.60×10-3 2.11×10-3 4 1.14×10-2 7.60×10-3 8.43×10-3Explanation / Answer
reaction is second order with respect to [NO]
first order with respect to [O2]
so rate law as follows
rate = K [NO]2 [O2]
K = rate / [NO]2 [O2]
K = (0.00105) / (0.00570)2(0.00380)
K = 0.00105 / 0.000000125
K = 8400 M-2 s-1
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