The rate of the reaction becomes twice when the concentration of reactant becomes $8$ times,then the order of the reaction is:

For the reaction $aA + bB \to$ product,the rate of reaction is given by $Rate = k[A]^3 [B]^0$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,the rate of reaction will be: (in $\times$)

Rate law for the reaction $aA + bB \rightarrow cC + dD$ is $r = k[A][B]$. The rate of reaction doubles if:

Consider the following reaction: $A \longrightarrow \text{Products}$. This reaction is completed in $100 \ min$. The rate constant of this reaction at $t_1 = 10 \ min$ is $10^{-2} \ min^{-1}$. What is the rate constant (in $min^{-1}$) at $t_2 = 20 \ min$?

What is the order and molecularity of the following reaction?
$NO_{2(g)} + NO_{2(g)} \longrightarrow 2NO_{(g)} + O_{2(g)}$

$2 \ FeCl_3 + SnCl_2 \rightarrow 2 \ FeCl_2 + SnCl_4$. This reaction is an example of: