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  4. 50.0 kg of N2(g) and 10.0 kg of H2(g) are mixed to produce NH3(g). Identify the limiting reagent in the production of NH3 in this situation.

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Q. $50.0\, kg$ of $N_{2(g)}$ and $10.0\, kg$ of $H_{2(g)}$ are mixed to produce $NH_{3(g)}$. Identify the limiting reagent in the production of $NH_3$ in this situation.

Some Basic Concepts of Chemistry

Solution:

The balanced chemical reaction is $N _2+3 H _2 \rightleftharpoons 2 NH _3$ From the above balanced equation, $1 mol$ of $N_{2(g)}$ reacts with 3 moles of $H _{2(g)}$.
$\therefore$ Moles of $N_2=\frac{50,000\, g }{28\, g\,mol ^{-1}}=1785.71 \,mol$
or, Moles of $H_2=\frac{10,000 g }{2.106\, g\, mol ^{-1}}=4960.3 \,mol$
$\therefore 1785.7\, mol$ of $N _2$ react with $3 \times 1785.7 \,mol =5357.1\, mol$
but we have $4960.3\, mol$ of $H _2$ only.
Therefore, $H _2$ is a limiting reagent.