For any reaction,the rate constant $K = 2.3 \times 10^{-5} \ mol^{-3/2} \ L^{3/2} \ S^{-1}$. The order of the reaction is . . . . . . .

The order of a reaction which has the rate expression $\frac{dc}{dt} = K[E]^{3/2}[D]^{3/2}$ is

In the reaction $2A + B \to A_2B$,if the concentration of $A$ is doubled and the concentration of $B$ is halved,then the rate of the reaction will:

For a given reaction $t_{1/2} = \frac{1}{k \cdot a}$,the order of reaction will be:

The following are the rate constants of two different reactions. What is the overall order of each reaction?
$(a)$ $2.1 \times 10^{-2} \ mol \ L^{-1} \ s^{-1}$
$(b)$ $4.5 \times 10^{-3} \ min^{-1}$

The reaction $2 A + B + C \longrightarrow D + E$ is found to be first order in $A$,second order in $B$,and zero order in $C$. What is the effect of increasing the concentration of all reactants twice?