Answer to Question #171267 in Chemistry for sdf

Question

1. Assume that the following reaction is in chemical equilibrium:

N2 (g) + 3H2 (g)  2NH3 (g) + heat

Use Le Chatelier’s principle to explain the effect each of the following changes will have upon the system – will the equilibrium shift towards the product or reactant side? Why?

1. If more hydrogen is added to the system, the equilibrium will shift to the… (right, left, or remains unchanged) and why?
2. If ammonia is removed from the system, the equilibrium will shift to the… (right, left, or remains unchanged) and why?
3. If nitrogen is removed from the system, the equilibrium will shift to the… (right, left, or remains unchanged) and why?
4. If the temperature is raised, the equilibrium will shift to the… (right, left, or remains unchanged) and why?
5. If the pressure of the system is decreased by doubling the total volume, the equilibrium will shift to the… (right, left, remains unchanged) and why?

 

Answer 1

N₂ (g) + 3H₂ (g) --> 2NH₃ (g) + heat

As heat is released, the reaction is exothermic.

1. If more hydrogen is added to the system, the equilibrium will shift to the right because an extra concentration of reactants needs to be used.

2. If ammonia is removed from the system, the equilibrium will shift to the right because the equilibrium must be restored.

3. If nitrogen is removed from the system, the equilibrium will shift to the left because the equilibrium must be restored.

4. If the temperature is raised, the equilibrium will shift to the left because the increased temperature will increase the amounts of products and the balance will shift toward reactants to restore equilibrium.

5. If the pressure of the system is decreased by doubling the total volume, the equilibrium will shift to the right because equilibrium shifts to side with a fewer number of gaseous molecules.