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
A		1	First order
B		2	Zero order
C
D

• A. $A-(1),B-(2),C-(2),D-(1)$
• B. $A-(2),B-(2),C-(1),D-(1)$
• C. $A-(2),B-(1),C-(1),D-(2)$
• D. $A-(1),B-(1),C-(2),D-(2)$

Answer 1

Answer: (A)

$A.\to (1)B.\to (2)C.\to (2)D.\to (1)$
For zero order reaction rate equation may be written as
$[R]=-kt+\left[R_0\right]$ ...(i)
Which denotes a straight line equation similar to $y=mx+c$
On transforming (i) $\frac{[R]-\left[R_0\right]}{t}=-k$
$k=\frac{\left[R_0\right]-[R]}{t}$

$k=$ Rate
Rate $=k\cdot [t{]}^0$
$\Rightarrow$ Rate $\propto [t{]}^0$

For a first order reaction $\frac{dx}{dt}\propto$ [concentration]
$\therefore$ Graph between rate and concentration may be drawn as
$k=\frac{2.303}{t}\log \frac{[R{]}_0}{[R]}$
$\frac{kt}{2.303}=\log \left[\frac{R^{\circ }}{R}\right]$
or $\frac{kt}{2.303}=\log [R{]}_0-\log [R]$
$\log [R]=\underset{\text{ Slope }}{\left(\frac{-k}{2.303}\right)}t+\underset{\text{ Intercept }}{\log [R{]}_0}$