The following graph shows how $T_{1/2}$ (half-life) of a reactant $R$ changes with the initial reactant concentration $a_0$. The order of the reaction will be:

The rate constant value for a reaction is $1.75 \times 10^2 \ L^2 \ mol^{-2} \ sec^{-1}$. The half-life period $t_{1/2} \propto$ . . . . . . .

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

If $a$ is the initial concentration and $n$ is the order of the reaction and the half-life period is $T$,then:

For a chemical reaction,the rate law is $\text{rate} = k[A]^2[B]$. If $[A]$ is doubled at constant $[B]$,the rate of reaction:

For the reaction $A + B \to$ products,doubling the concentration of $A$ the rate of the reaction is doubled,but on doubling the concentration of $B$ the rate remains unaltered. The overall order of the reaction is: