Making+Ammonia+-+The+Haber+process

__Haber Process__
This is the process by which ammonia (NH3) is produced. The equation for this reaction is... The symbol that you see in the middle means it is a reversible reation, so the product can decompose back into the reactants. So optimum conditions must be selected to get the greatest yield. When the forward and backward reactions are the same, it is said to be in a state of equilibrium.


 * ~ Condition ||~ Effect ||
 * Pressure || Increasing this will improve the yield because the forward reaction reduces pressure. However, putting up the pressure too far is impractical and becomes too expensive because special instruments must be used to withstand the forces. ||
 * Temperature || A higher yield can be obtained by using a low temperature since the forward reaction produces heat, but this also will make the reaction slower, and less profitable so a temperature of about 450°C is used. ||
 * Catalyst || The haber process makes use of iron to speed up the reaction - but this doesn't improve the yield ||

The conditions of the Haber process must be finely balanced to reach a combination of highest yield and fastest reaction, this is very important because getting this right will make sure this industrial process is as profitable as possible.