![\dfrac{d[D]}{dt}=k_3[B][C] --- (1)](/tpl/images/1136/4952/b9e57.png)
![\dfrac{d[B]}{dt}=k[A] -k_2[B] -k_3[B][C]](/tpl/images/1136/4952/9c7ee.png)
![\dfrac{d[B]}{dt}=0](/tpl/images/1136/4952/07994.png)
![k_1[A]-k_2[B]-k_3[B][C] = 0](/tpl/images/1136/4952/5db8e.png)
![[B] = \dfrac{k_1[A]}{k_2+k_3[C]}](/tpl/images/1136/4952/be881.png)
![\mathbf{\dfrac{d[D]}{dt}= \dfrac{k_3k_1[A][C]}{k_2+k_3[C]}}](/tpl/images/1136/4952/f5cf3.png)
![\dfrac{d[D]}{dt} = \dfrac{k_3k_1[A][C]}{k_3[C]}= k_1A \ \ \text{first order}](/tpl/images/1136/4952/eb417.png)
![\dfrac{d[D]}{dt} = \dfrac{k_3k_1[A][C]}{k_2}= \dfrac{k_1k_3}{k_2}[A][C] \ \ \text{second order}](/tpl/images/1136/4952/5482d.png)
How to set up the rate expressions for the following mechanism?
A → B k1
B → A k2
B...
Chemistry, 22.02.2021 19:10 nikitakhrabkov123
How to set up the rate expressions for the following mechanism?
A → B k1
B → A k2
B+C → D k3
If the concentration of B is small compared with the concentrations of A, C, and D, the steady-state approximation may be used to derive the rate law. Derive the rate law, and show that this reaction may follow the first-order equation at high pressures and the second-order equation at low pressures.
Answers: 2
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