The time required for a definite fraction of a reaction to complete is inversely proportional to the initial concentration of the reactant. Find the order of the reaction.

For a hypothetical reaction,$A \rightarrow C$. The mechanism is: $A \underset{k_2}{\stackrel{k_1}{\rightleftharpoons}} B$ (Fast),$A + B \xrightarrow{k_3} C$ (Slow). The rate law for this reaction is:

The unit of the rate constant for a second-order reaction is ......

The rate equation for the reaction $2A + B \longrightarrow \text{products}$ is $\text{rate} = k[A][B]^2$. If $k$ at $T \, K$ is $5.0 \times 10^{-6} \, mol^{-2} \, L^2 \, s^{-1}$,the initial rate of the reaction,when $[A] = 0.05 \, mol \, L^{-1}$ and $[B] = 0.1 \, mol \, L^{-1}$ is:

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:

Write the general equation of a reaction and explain what the order of reaction is. What are its possible values?