Product Chemistry Example 5

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Example 5

hard
In the Haber process, N2+3H2⇌2NH3\text{N}_2 + 3\text{H}_2 \rightleftharpoons 2\text{NH}_3, calculate the mass of ammonia (NH3\text{NH}_3) produced from 56.056.0 g of nitrogen gas reacting with excess hydrogen. (N = 14.0114.01, H = 1.008 g/mol1.008\,\text{g/mol})

Solution

  1. 1
    Moles of N2=56.028.02=2.00 mol\text{N}_2 = \frac{56.0}{28.02} = 2.00\,\text{mol}.
  2. 2
    From the equation: 1 mol N2\text{N}_2 → 2 mol NH3\text{NH}_3. So moles of NH3=2.00×2=4.00 mol\text{NH}_3 = 2.00 \times 2 = 4.00\,\text{mol}.
  3. 3
    Molar mass of NH3=14.01+3(1.008)=17.03 g/mol\text{NH}_3 = 14.01 + 3(1.008) = 17.03\,\text{g/mol}. Mass =4.00×17.03=68.1 g= 4.00 \times 17.03 = 68.1\,\text{g}.

Answer

68.1 g of NH368.1\,\text{g of NH}_3
The Haber process is one of the most important industrial reactions, producing ammonia for fertilizers. Calculating theoretical product mass follows the standard stoichiometric pathway: grams → moles → ratio → moles → grams.

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