Consider the following system at equilibrium: N₂ (g) + 3 H₂ (g) $\rightarrow$ 2 NH₃ (g) + 92. 94 kJ
Which of the following changes will shift the equilibrium to the right?
1) Increasing the temperature 2. Decreasing the temperature
3) Increasing the volume 4. Decreasing the volume
5) Removing some NH₃ 6. Adding some NH₃
7) Removing some N₂ 8. Adding some N₂

Question

Consider the following system at equilibrium: N₂ (g) + 3 H₂ (g)

\rightarrow

2 NH₃ (g) + 92. 94 kJ
Which of the following changes will shift the equilibrium to the right?
1) Increasing the temperature 2. Decreasing the temperature
3) Increasing the volume 4. Decreasing the volume
5) Removing some NH₃ 6. Adding some NH₃
7) Removing some N₂ 8. Adding some N₂

Quizplus · Accepted Answer

The reaction is endothermic, so decreasing the temperature (2) will shift the equilibrium to the left, not the right. Increasing the volume (3) will shift the equilibrium to the side with more moles of gas, which is the left side in this case. Removing some of the product, NH₃ (5), will shift the equilibrium to the right to produce more product. Adding more reactant, N₂ (8), will also shift the equilibrium to the right to consume the added reactant.

Consider the Following System at Equilibrium: N2 (G) + 3 →\rightarrow→

Consider the Following System at Equilibrium: N₂ (G) + 3 $\rightarrow$