For reaction $\mathrm{A}+\mathrm{B} \rightarrow$ product, rate of reaction is $3.6 \times 10^{-2} \mathrm{sec}^{-1}$. When $[\mathrm{A}]=0.2 \mathrm{moldm}^{-3}$ and $[B]=0.1 \mathrm{moldm}^{-3}$, calculate rate constant of reaction if reaction is first order in A and second order is B ?

For a reaction $\mathrm{r}=\mathrm{k}[\mathrm{A}][\mathrm{B}]^2$, if concentration of $A$ is doubled the rate of reaction

For the reaction

$$\begin{aligned} & 2 \mathrm{NO}_{(\mathrm{s})}+2 \mathrm{H}_{2(\mathrm{~g})} \longrightarrow \mathrm{N}_{2(\mathrm{~g})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{s})} \\\\ & \text { rate }=\mathrm{k}[\mathrm{NO}]^2\left[\mathrm{H}_2\right] . \end{aligned}$$

What is the order of reaction with respect to $\mathrm{H}_2$ and overall order of reaction respectively?

Which among the following statements is NOT true about rate constant?