Rate Law Question?

2018-01-12 9:16 am
Which of the following expressions for the rate law (either differential or integrated) are completely consistent with second-order reactions.

k[NO2] = -d[NO2]/dt

[NO2] = [NO2]0 - kt

[NO2] = 1/(kt + 1/[NO2]0)

-d[NO2]/dt = k[NO2]2

k[NO2]2 = d[NO]/dt
更新1:

Equation: NO2(g) + CO(g) --> NO(g) + CO2(g)

回答 (1)

2018-01-12 2:34 pm
✔ 最佳答案
For k[NO₂] = -d[NO₂]/dt, i.e.
-d[NO₂]/dt = k[NO₂]
This is the differential form of a FIRST-order reaction.

For [NO₂] = [NO₂]ₒ - kt, i.e.
[NO₂]ₒ - [NO₂] = kt
This is the integrated form of a ZERO-order reaction.

For [NO₂] = 1/[kt + (1/[NO₂]ₒ)], i.e.
kt + (1/[NO₂]ₒ) = 1/[NO₂]
(1/[NO₂]) - (1/[NO₂]ₒ) = kt
This is the integrated from of a SECOND-order reaction.

For -d[NO₂]/dt = k[NO₂]²
This is the differential from of a SECOND-order reaction.

For k[NO₂]² = d[NO]/dt, i.e.
d[NO]/dt = k[NO₂]²
This is the differential from of a SECOND-order reaction.

The three answers :
[NO₂] = 1/[kt + (1/[NO₂]ₒ)]
-d[NO₂]/dt = k[NO₂]²
k[NO₂]² = d[NO]/dt


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