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Question
Match the graph given in Column I with the order of reaction given in Column II. More than one item in Column I may link to the same item of Column II.
| Column I | Column II | |
| (i) |  |
|
| (ii) |  |
(a) 1st order |
| (iii) |  |
(b) Zero-order |
| (iv) |  |
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Solution
| Column I | Column II | |
| (i) | |
(a) 1st order |
| (ii) | |
(b) Zero-order |
| (iii) | |
(b) Zero order |
| (iv) | |
(a) 1st order |
Explanation:
For zero order reaction rate equation may be written as [R] = – kt + [R0]
Which denotes a straight line equation similar to y = mx + c
On transmitting (i) `([R] - [R_0])/t = - k`
`k = ([R_0] - [R])/t`
k = Rate
Rate = `k.[t]^0`
Rate `oo [t]^0`
For a first order reaction `(dx)/(dt) oo` [concentration]
∴ Graph between rate and concentration may be drawn as
`k = 2.303/t log ([R]_0)/([R])`
`(kt)/2.303 = log ([R]_0)/([R])`
`(kt)/2.303 = log[R_0] - log[R]`
\[\ce{log[R] = \underset{(Slope)}{\frac{-k}{2.303}} t + \underset{(Intercept)}{log[R]_0}}\]
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