Answer to Question #170799 in General Chemistry for 8795

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

$N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)} + Heat$

1. The equilibrium will shift to the right, to produce more products

2. The equilibrium will shift to the right too, to.produce more ammonia

3. The equilibrium will shift to the left, to produce more hydrogen.

4. The equilibrium will shift to the left because the reaction is exothermic

5. The pressure will shift to the left due to the lesser pressure of the products, causing decomposition of the product.