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<chem> 3H2(g) + N2(g) <=> 2NH3(g) </chem>
: The [[Chemical Reaction|reaction]] in the [[Haber Process]] will reach a state of [[Dynamic Equilibrium|dynamic equilibrium]] with an [[Equilibrium Position(Chemistry)|equilibrium position]] which can be changed by altering the [[temperature]] or [[pressure]] of the [[Reaction Mixture|reaction mixture]].
: The [[Yield (Chemistry)|yield]] can be improved by increasing the [[pressure]] inside the [[Reaction Vessel|reaction vessel]] which favours the forward [[Chemical Reaction|forward reaction]].
: The [[Haber Process]] is essential to modern agriculture as it produces [[Nitrogen]] based [[fertiliser]]s for crops. Without this the [[soil]] would run out of [[Nitrate]]s and [[plant]]s would not longer be able to [[growth|grow]].
===(Higher) Iron Catalyst and the Haber Process===
: The [[Iron]] [[catalyst]] increases the [[Rate of Reaction|rate of reaction]].
: However, this works for both the [[Forward Reaction|forward]] and [[Back Reaction|back reaction]] so it does not affect the [[Equilibrium Position(Chemistry)|equilibrium position]].
===(Higher) Pressure and the Haber Process===
: Using the [[Balanced Symbol Equation|balanced symbol equation]] for this [[Chemical Reaction|reaction]]:
: <chem> 3H2(g) + N2(g) <=> 2NH3(g) </chem>
: It can be seen that 4 [[Mole]]s of [[reactant]]s is needed to [[product|produce]] 2 [[Mole]]s of [[product]]s. This means a higher [[pressure]] will force the [[Equilibrium Position(Chemistry)|equilibrium position]] to favour the [[product]]s over the [[reactant]]s as they take up less [[Volume (Space)|volume]].
===(Higher) Temperature and the Haber Process===