Assume 100 g sample. For every 100 g sample, we can obtain the mass of nitrogen which is numerically equal to the percent nitrogen content.

For NH_{3}:

$\mathbf{mass}\mathbf{}\mathbf{N}\mathbf{=}\mathbf{100}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{NH}}_{\mathbf{3}}}\left(\frac{1\overline{)\mathrm{mol}{\mathrm{NH}}_{3}}}{17.031\overline{)g{\mathrm{NH}}_{3}}}\right)\left(\frac{1\overline{)\mathrm{mol}N}}{1\overline{)\mathrm{mol}{\mathrm{NH}}_{3}}}\right)\left(\frac{14.01gN}{1\overline{)\mathrm{mol}N}}\right)\mathbf{=}$**82.26 g N**

Most fertilizers consist of nitrogen-containing compounds such as NH_{3}, CO(NH_{2} )_{2}, NH_{4} NO_{3}, and (NH_{4} )_{2} SO_{4}. Plants use
the nitrogen content in these compounds for protein synthesis.

Which fertilizer has the highest nitrogen content?

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