The haber process

Why is the product production continuous

Decreaseing nh3 shifts equilibrium and allows more to be made
Unused n2 and h2 constantly recycled back into system, increasing reactants causes equilibrium to shift and make more nh3

Nitrogen source

Air

Hydrogen source

CH4 or steam

Haber process conditions

2atmospheres, 450 degrees, iron catalyst

equation for haber process

N2 + 3H2 = 2NH3
E=-VE

Forward reaction heat

Exothermic

reverse reaction heat

Endothermic

Increase in heat effects

Shift's equilibrium to left so endothermic reaction uses up the heat

Increase in pressure effects

Shifts equilibrium to right. Fewer moles on products side

Condition pressure

200 atm

Temperature conditions

380-450 °C

Catalyst and effects

Iron
Increases rate of reaching equilibrium at a lower temperature
Acts as a surface where N2 and H2 react

NH3 extraction

Equilibrium mixture is cooled. Allows NH3 to liquify and can be removed.
Decreaseing nh3 shifts equilibrium and allows more to be made
Unused n2 and h2 constantly recycled back into system, increasing reactants causes equilibrium to shift and make more nh3