$3\mathrm{.}9104g$ sample of a compound made of carbon, hydrogen, nitrogen, and oxygen is burned completely. $3\mathrm{.}820gC{O}_2$ and $3\mathrm{.}125g{H}_{2}O$ are produced. Analysis of nitrogen showed that the compound contains $46\mathrm{.}62\%$ by mass nitrogen.

Use the following molar masses $($if needed$)$ for your calculations:

$C{O}_2=44\mathrm{.}01\frac{g}{m}ol$

$H_{2}O=18\mathrm{.}02\frac{g}{m}ol$

$H=1\mathrm{.}01\frac{g}{m}ol$

$C=12\mathrm{.}01\frac{g}{m}ol$

$O=16\mathrm{.}00\frac{g}{m}ol$

$N=14\mathrm{.}01\frac{g}{m}ol$

What is the empirical formula?