What is rate constant of a first order reaction if 0.08 mole of reactant reduces to 0.02 mole in 23.03 minute?

Which of the following statements is NOT true for a reaction having rate law $$\mathrm{r}=\mathrm{k}\left[\mathrm{H}_2\right]\left[\mathrm{I}_2\right]$$ ?

For the reaction $$\mathrm{N}_{2(\mathrm{~g})}+3 \mathrm{H}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{NH}_{3(\mathrm{~g})}$$, what is the relation between $$\frac{\mathrm{d}\left[\mathrm{N}_2\right]}{\mathrm{dt}}$$ and $$\frac{\mathrm{d}\left[\mathrm{H}_2\right]}{\mathrm{dt}}$$ ?

For a reaction $$\mathrm{A} \rightarrow$$ product, rate constant is $$2 \times 10^{-2} \mathrm{~s}^{-1}$$. The initial concentration of $$\mathrm{A}$$ is 1.0 mol dm$${ }^{-3}$$. What is the value of $$\log \frac{1}{[\mathrm{~A}]_{\mathrm{t}}}$$ after 100 seconds?