Identify all of the following three changes that would shift the equilibrium of the haber [hah-bur] process to the right: a) adding hydrogen gas; b) adding an inert gas; c) increasing the volume of the container at constant temperature.

a).Adding hydrogen gas : Forward direction

b) Adding an inert gas

c) Increasing the volume of the container:Backward direction

Explanation:

According to Le-Chatelier's principle = Any disturbance is created in the equilibrium , it will shift the equilibrium in such a way to reduce disturbance.

This disturbance can be : Change in concentration , pressure, temperature , Addition of gas etc.

Temperature : when temperature is increased for endothermic reaction . The equilibrium shift in forward. For exothermic reaction , on increasing temperature ,equilibrium  shift backward.

Pressure : On increasing pressure the equilibrium shifts towards less number of gaseous molecules.

Volume : Since volume varies inversely with pressure . It's effect is opposite to that produced by pressure change i.e On increasing Volume the equilibrium shifts towards more number of gaseous molecules.

On Addition of Inert gas : The equilibrium shift toward the side where more gaseous molecules are present.

Concentration : On increasing concentration , the equilibrium will shift such that the substance added get removed .

Haber Process  :

This is exothermic reaction (H = negative)

Molecules of gases are more on left side(reactants) than right side(product)

a) Adding hydrogen gas :

According to Le-Chatelier's principle ,The equilibrium will shift in a direction where the  Hydrogen gas is consumed (removed)

Hence Equilibrium shift in forward direction

b) Adding an inert gas : There are two situation

c) Increasing the volume of the container:

If total Volume is increased, the number of molecules per unit volume decrease.In order to maintain the equilibrium constant , the equilibrium shift  in direction where there is increase in number of molecule(Le-Chatelier's).

In this case Backward direction.

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