For a reaction of order $n$,the unit of the rate constant is :

When the concentration of a reactant,$A$,in a reaction $A \to \text{Products}$ is doubled,the rate of reaction increases seven times. The order of the reaction is between:

Which of the following is an example of a second-order reaction?

For the reaction $A \to \text{Products}$,the rate of reaction becomes one-fourth when the concentration of $A$ is halved. What is the order of the reaction?

$A$ substance undergoes first-order decomposition. The decomposition follows two parallel first-order reactions as:
$A \xrightarrow{k_1} B$ $k_1 = 1.26 \times 10^{-4} \ s^{-1}$
$A \xrightarrow{k_2} C$ $k_2 = 3.8 \times 10^{-5} \ s^{-1}$
The percentage distribution of $B$ and $C$ are:

The rate of the reaction $CCl_3CHO + NO \to CHCl_3 + NO + CO$ is given by $Rate = K [CCl_3CHO] [NO]$. If concentration is expressed in $mol \ L^{-1}$,the units of $K$ are: