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)

Answer 1

	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]`

\[\ce{log[R] = \underset{(Slope)}{\frac{-k}{2.303}} t +  \underset{(Intercept)}{log[R]_0}}\]