Find the rate of formation of $$\mathrm{NO}_{2(\mathrm{~g})}$$ in the following reaction.

$$\begin{aligned} & 2 \mathrm{~N}_2 \mathrm{O}_{5(\mathrm{~g})} \rightarrow 4 \mathrm{NO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})} \\ & {\left[\frac{-\mathrm{d}\left[\mathrm{N}_2 \mathrm{O}_5\right]}{\mathrm{dt}}=0.02 \mathrm{~mol} \mathrm{~dm}^{-3}\right]} \end{aligned}$$

Calculate the rate constant of the first order reaction if $$20 \%$$ of the reactant decomposes in 15 minutes.

Which from following is the slope of the graph of $$[\mathrm{A}]_{\mathrm{t}}$$ versus time for zero order reaction?

A first order reaction takes 23.03 minutes for $$20 \%$$ decomposition. Calculate its rate constant.