For the reaction $\mathrm{A}+\mathrm{B} \rightarrow \mathrm{C}$, the following data were obtairied…
For the reaction $\mathrm{A}+\mathrm{B} \rightarrow \mathrm{C}$, the following data were obtairied
$\begin{array}{llll}
\text{Exp} & {\text{Initial concentration}} & \text{Initial rate} \\
& [A]_{M} & [B]_{M} & (M \, \text{min}^{-1}) \\
1. & 0.1 & 0.1 & 1.0 \times 10^{-4} \\
2. & 0.1 & 0.3 & 9.0 \times 10^{-4} \\
3. & 0.3 & 0.3 & 2.7 \times 10^{-3}
\end{array}$
The order of reaction with respect to $A$ and $B$ are respectively
1,2
2,1
1.5,1.5
0,3
Solution
When initial concentration of A is kept constant and that of B is changed (tripled), the rate of the reaction increase by 9 times.
Thus, the order of the reaction will be $\alpha$ with respect to $B$. When the concentration of B is kept constant and that of $\mathrm{A}$ is increased by 3 times, the rate of the reaction increases by 3 times too.
Thus, the order of the reaction is 1 with respect to $A$.