Chemistry, 13.08.2019 05:20, julialombardo53
The following mechanism has been suggested for the reaction between nitrogen monoxide and oxygen: no(g) + no(g) โ n2o2(g) (fast) n2o2(g) + o2(g) โ 2no2(g) (slow) according to this mechanism, the experimental rate law is a. second-order in no and zero-order in o2. b. second-order in no and first-order in o2. c. first-order in no and second-order in o2. d. first-order in no and first-order in o2. e. first-order in no and zero-order in o2.
Answers: 3
![\rm 2NO\xrightarrow[k_{-1}]{k_{1}}N_{2}O_{2} \, (fast)\\\rm N_{2}O_{2} + O_{2}\xrightarrow{k_{2}} 2NO_{2} \, (slow)](/tpl/images/0174/8111/fd274.png)
![-\dfrac{\text{d[NO]} }{\text{d}t} = k_{1}[\text{NO]}^{2} - k_{-1} [\text{N}_{2}\text{O}_{2}]^{2}\\\\\rm -\dfrac{\text{d[N$_{2}$O$_{2}$]}}{\text{d}t} = -\dfrac{\text{d[O$_{2}$]}}{\text{d}t} = k_{2}[ N_{2}O_{2}][O_{2}] - k_{1} [NO]^{2}\\\\\dfrac{\text{d[NO$_{2}$]}}{\text{d}t}= k_{2}[ N_{2}O_{2}][O_{2}]](/tpl/images/0174/8111/962f7.png)
![\rm k_{1}[NO]^{2} = k_{-1} [N_{2}O_{2}]\\\\\rm [N_{2}O_{2}] = \dfrac{k_{1}}{k_{-1}}[NO]^{2}](/tpl/images/0174/8111/3a2a1.png)
![\rm \dfrac{\text{d[NO$_{2}$]}}{\text{d}t}= \dfrac{k_{2}k_{1}}{k_{-1}}[NO]^{2} [O_{2}] = k[NO]^{2} [O_{2}]](/tpl/images/0174/8111/64b85.png)
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The following mechanism has been suggested for the reaction between nitrogen monoxide and oxygen: n...
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