$$\(2 \mathrm{~N}_{2}(\mathrm{~g})\)$$ reacts with $$\(\mathrm{H}_{2}(\mathrm{~g})\)$$ in the Haber process, as shown in reaction 1. $$\[ \text { reaction } 1 \quad \mathrm{~N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g}) \quad \Delta H=-\mathrm{x} \mathrm{kJ} \mathrm{mol}{ }^{-1} \]$$ Table 2.1 shows the different conditions used to produce three equilibrium mixtures, $$\(\mathbf{A}, \mathbf{B}\)$$ and $$\(\mathbf{C}\)$$.

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