Changes

{{#ev:youtube|https://www.youtube.com/watch?v=o1_D4FscMnU}}: In the [[Haber Process]] [[Nitrogen]] and [[Hydrogen]] [[gas]] are passed over an [[Iron]] [[catalyst]] at 450°C and a [[Pressure]] of 20,200,000[[Pascal|Pa]] (200 times normal [[Atmospheric Pressure|atmospheric pressure]]).

<chemmath> 3H23H_2(g) + N2N_2(g) <=> 2NH3⇌ 2NH_3(g) </chemmath>: 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 [[Haber Process]] is essential to modern [[agriculture]] as it produces [[Nitrogen]] based [[fertiliser]]s for [[crop]]scrops. 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]]:: <chemmath> 3H23H_2(g) + N2N_2(g) <=> 2NH3⇌ 2NH_3(g) </chemmath>: 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===: The [[temperature]] affects both the [[Rate of Reaction|rate of reaction]] and the [[Equilibrium Position(Chemistry)|equilibrium position]].