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.

Answer 1

$A.\to \left(1\right)B.\to \left(2\right)C.\to \left(2\right)D.\to \left(1\right)$

For zero order reaction rate equation may be written as
$\left[R\right]=-kt+\left[R_0\right]$ ....(i)

which denotes a striaght line equation similar to y=m x + c

On transforming (i) $\frac{\left[R\right]-\left[R_0\right]}{t}=-kk=\frac{\left[R_0\right]-\left[R\right]}{t}$

k=Rate

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

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