Identify the order of the following reaction: $2 NO_{2(g)} \longrightarrow 2 NO_{(g)} + O_{2(g)}$

For the reaction $2NOBr(g) \rightarrow 2NO(g) + Br_2(g)$, the rate law is $r = k[NOBr]^2$. If the rate constant $k = 1.62 \times 10^{-2} \text{ L mol}^{-1} \text{ s}^{-1}$ and the concentration of $[NOBr] = 2 \times 10^{-3} \text{ mol L}^{-1}$, what is the rate of reaction?

Which of the following is an example of a second-order reaction?

The rate law for the reaction $A + 2B \rightarrow C + 2D$ is given by:

At what concentration of the reactant (in $M$) are the rate constants for first-order,second-order,and third-order reactions equal?

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