Question on Haber process equilibrium?

You can shift the equilibrium toward the product by:

1. removing ammonia

2. adding more reactant(s), preferably in the ratio 1 volume of nitrogen for every 3 volumes of hydrogen

Your reading "somewhere" sounds bogus. If it is a reactant, more of it produces more product as long as there is already enough of the other reactant to react with it.

At constant pressure and temperature, the equilibrium position would shift to the right by adding the reactant(s) (N₂ and/or H₂) or removing the product (NH₃).

The equilibrium position would shift to the right by adding an excess of H₂. However, we often add an excess of N₂ instead. This is because the cost of N₂ is much lower than that of H₂. N₂ is made by fraction distillation of liquefied air, while H₂ is made by the catalytic hydration of a fraction of petroleum.

increase total pressure or increase partial pressure of reactants, continuously remove the product ammonia as soon as it is formed, use lower temperature and a develop a new catalyst that will allow to use lower temperatures. The current catalyst compels to use a temperature of at least 450degC and the pressure adds to capital and operating c costs.