The half-life of a reaction is found to be inversely proportional to the cube of its initial concentration. The order of the reaction is:

........ of a reaction cannot be determined experimentally.

For the reaction $A + 2B \to C$,the rate is given by $R = k[A][B]^2$. The order of the reaction is:

For the reaction between $A$ and $B$,the initial rate of reaction $(r_0)$ was measured for different initial concentrations of $A$ and $B$ as given below. Determine the order of the reaction with respect to $A$ and $B$ respectively.

$[A] / mol \ L^{-1}$	$0.2, 0.2, 0.4$
$[B] / mol \ L^{-1}$	$0.3, 0.1, 0.05$
$r_0 / mol \ L^{-1} s^{-1}$	$5.0 \times 10^{-5}, 5.0 \times 10^{-5}, 1.4 \times 10^{-4}$

The rate of a reaction depends upon the

If the half-life of a reaction is halved when the initial concentration of the reactant is doubled,what is the order of the reaction?