The reaction is second order in NO and first order in O2. When and , the observed rate
Chapter 20, Problem 14.99(choose chapter or problem)
The reaction \(2 \mathrm{NO}(g)+\mathrm{O}_2(g) \longrightarrow 2 \mathrm{NO}_2(g)\) is second order in NO and first order in \(\mathrm{O}_2\). When NO] = 0.040 M and \(\left[\mathrm{O}_2\right]\) = 0.035 M, the observed rate of disappearance of NO is \(9.3 \times 10^{-5} \mathrm{M} / \mathrm{s}\).
(a) What is the rate of disappearance of \(\mathrm{O}_2\) at this moment?
(b) What is the value of the rate constant?
(c) What are the units of the rate constant?
(d) What would happen to the rate if the concentration of NO were increased by a factor of 1.8?
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