Ammonium nitrate $((\mathrm{NH} 4 \mathrm{NO} 3,80.04 \mathrm{~g} / \mathrm{mol})$ is a fertilizer that can help enrich the nitrogen content of soil. A farmer wants to fertilize her field with $625 \mathrm{~kg}$ of nitrogen (N). How many grams of ammonium nitrate should she use?

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***A*** ∻Key Concept∻ ⚹Molar Mass and Stoichiometry⚹ ∻Explanation∻ ⚹To find the amount of ammonium nitrate needed, we use the molar mass of ammonium nitrate and the stoichiometry of nitrogen in the compound to convert from mass of nitrogen desired to mass of ammonium nitrate required.⚹◊What is the molecular weight of ammonium nitrate ($NH_4NO_3$)?⍭ Generate me a similar question◊

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