In a first order reaction $60 \%$ of the reactant converts into product in 45 minute. Calculate rate constant of the reaction.

For the reaction,

$$\mathrm{CH}_3 \mathrm{Br}_{(\mathrm{aq})}+\mathrm{OH}_{(\mathrm{aq})}^{-} \longrightarrow \mathrm{CH}_3 \mathrm{OH}_{(\mathrm{aq})}+\mathrm{Br}_{(\mathrm{aq})}^{-}$$

rate of consumption of $\mathrm{OH}_{(\mathrm{aq})}^{-}$is $\mathrm{x} \mathrm{mol} \mathrm{dm}{ }^{-3} \mathrm{~s}^{-1}$ What is the rate of formation of $\mathrm{Br}_{(9 q)}^{-}$?

For the reaction,

$$\mathrm{H}_{2(g)}+\mathrm{Br}_{2(8)} \longrightarrow 2 \mathrm{HBr}_{(\mathrm{g})}, \mathrm{r}=\mathrm{k}\left[\mathrm{H}_2\right]\left[\mathrm{Br}_2\right]^{\frac{1}{2}}$$

What is the molecularity and order of reaction respectively?

Which of the following is true for a reaction as per coliision theory?