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===Meaning===
The [[Haber Process]] is a process used to [[product|produce]] [[Ammonia]] from [[Nitrogen]] [[gas]].
===About the Haber Process===
: In the [[Haber Process]] [[Nitrogen]] and [[Hydrogen]] [[gas]] are passed over an [[Iron]] [[catalyst]] at 450°C and a [[Pressure]] of 20,200,000[[Pa]] (200 times normal [[Atmospheric Pressure|atmospheric pressure]]).
: The [[Chemical Reaction|reaction]] in the [[Haber Process]] is a [[Reversible Reaction|reversible reaction]]:
Hydrogen + Nitrogen ⇌ Ammonia
<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|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 [[crop]]s. Without this the [[soil]] would run out of [[Nitrate]]s and [[plant]]s would not longer be able to [[growth|grow]].
===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]] to favour the [[product]]s over the [[reactant]]s as they take up less [[Volume (Space)|volume]].
===Temperature and the Haber Process===
: The [[temperature]] affects both the [[Rate of Reaction|rate of reaction]] and the [[Equilibrium Position]].
: A higher [[temperature]] increases the [[Rate of Reaction|rate of reaction]] because it causes the [[particle]]s of [[reactant]] to [[Collision Theory|collide]] more frequently.
: A higher [[temperature]] favours the [[Back Reaction|back reaction]] because the [[Forward Reaction|forward reaction]] is [[exothermic]] and the [[Back Reaction|back reaction]] is [[endothermic]].
: To optimise the [[Rate of Reaction|rate of reaction]] and the [[Forward Reaction|forward reaction]] the optimum [[temperature]] is 450°C. This [[temperature]] [[product|produces]] the best [[Yield (Chemistry)|yield]] in the shortest [[time]].