The rate of reaction $A + 2B \to 3C$ becomes $72\, times$ when concentration of $A$ is tripled and concentration of $B$ is doubled then the order of reaction with respect to $A$ and $B$ respectively is
The rate of reaction $A + 2B \to 3C$ becomes $72\, times$ when concentration of $A$ is tripled and concentration of $B$ is doubled then the order of reaction with respect to $A$ and $B$ respectively is
- A
$1, 2$
- B
$2, 3$
- C
$3, 2$
- D
$2, 2$
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$1.$ $\frac {5}{2}$ order
$2.$ $n$ order
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The half life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $'p_0'$ as follows :
$\begin{array}{|l|l|l|} \hline P_0\,\,(mmHg) & 250 & 300 \\ \hline t_{1/2}\,\,(minutes) & 135 & 112.5 \\ \hline \end{array}$
The order of reaction is -
The half life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $'p_0'$ as follows :
$\begin{array}{|l|l|l|} \hline P_0\,\,(mmHg) & 250 & 300 \\ \hline t_{1/2}\,\,(minutes) & 135 & 112.5 \\ \hline \end{array}$
The order of reaction is -