(Solved): In the following chemical reaction between \( \mathrm{H}_{2} \) and \( \mathrm{N}_{2} \) to produce ...

In the following chemical reaction between \( \mathrm{H}_{2} \) and \( \mathrm{N}_{2} \) to produce \( \mathrm{NH}_{3} \), what is the mass of \( \mathrm{N}_{2} \) needed to completely react with \( 0.66 \mathrm{~g} \) of \( \mathrm{H}_{2} \) to produce \( 3.71 \mathrm{~g}^{2} \) of \( \mathrm{NH}_{3} \) ? \[ 3 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{N}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{NH}_{3}(\mathrm{~g}) \] (i) Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal e.g. \( 2.5 \mathrm{e} 5 \) for \( 2.5 \) \( \left.\times 10^{5}\right) \)