equilibrium shift using haber process

Question

Using the Haber process (produces NH3 from Nitrogen and hydrogen gas) give 2 situations which would shift the equilibrium to the right and give 2 examples/situations which would shift the equilibrium to the left

Answer 1

N2 (g) + 3 H2 (g) < —> 2 NH3 (g) 

 

A system at equilibrium will respond to a stressor or change in its environment by adjusting in a way that maintains its Equilibrium. One way it does that is by keeping the relative ratio of reactnts and product the same. If something is removed, the system shifts to make more of it. If something is added, the system shifts to use up the “excess” and make more of the molecules on the other side of the reaction.

 

Therefore, the equilibrium would shift to the right in response to one of the following changes in concentration:

 

a) adding more reactant molecules, which will then come together give more of the NH3 product, thus driving the reaction in the forward direction

b) remove product molecules, which will again drive the reaction in the forward direction to replace them

 

Following that same understanding, the equilibrium would shift to the left in response to one of the following changes in concentration:

 

A) adding more product molecules

b) removing reactant molecules 

 

because this is a gaseous equilibriu, we could also manipulate the equilibrium position through changes in pressure. when pressure is increased, the equilibrium will shift in a direction that produces fewer moles of gas, thus relieving the added pressure. When pressure is reduced, the equilibrium will shift in a direction that produces more moles of gas, in an attempt to maintain its original pressure.

 

therefore, to shift the equilibrium to the right for this system, we would increase pressure. To shift the equilibrium to the left, we would decrease pressure.