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

For a gaseous reaction,the rate is given by $Rate = k [A] [B]$. If the volume of the container is reduced to $1/4$ of its initial volume,the rate of the reaction will become how many times the initial rate?

The rate constant for the reaction, $2 \,N_2O_{5(g)} \rightarrow 2 \,N_2O_{4(g)} + O_{2(g)}$ is $4.98 \times 10^{-4} \,s^{-1}$. What is the order of the reaction?

Half-life of a reaction is found to be inversely proportional to the fifth power of its initial concentration,the order of reaction is

Which of the following options correctly represents the relationship between $t_{7/8}$ and $t_{1/2}$ where $t_{7/8}$ represents the time required for the concentration to become $1/8$ of the original for a reaction of order $n$?