Given the reaction below, explain how the equilibrium would be reestablished after each of the following stresses are applied.
4NH₃(g) + 3O₂(g) 2N₂(g) + 6H₂O(g) H^° = -12.0 kJ/mol
a) Addition of water
b) Removal of ammonia
c) Increase of the volume of the container
d) Lowering of the reaction temperature

Question

Given the reaction below, explain how the equilibrium would be reestablished after each of the following stresses are applied.
4NH₃(g) + 3O₂(g)

Given the reaction below, explain how the equilibrium would be reestablished after each of the following stresses are applied. 4NH<sub>3</sub>(g) + 3O<sub>2</sub>(g) 2N<sub>2</sub>(g) + 6H<sub>2</sub>O(g) H<sup>°</sup> = -12.0 kJ/mol a) Addition of water b) Removal of ammonia c) Increase of the volume of the container d) Lowering of the reaction temperature

2N₂(g) + 6H₂O(g) Given the reaction below, explain how the equilibrium would be reestablished after each of the following stresses are applied. 4NH3(g) + 3O2(g) 2N2(g) + 6H2O(g) H° = -12.0 kJ/mol a) Addition of water b) Removal of ammonia c) Increase of the volume of the container d) Lowering of the reaction temperature

H^° = -12.0 kJ/mol
a) Addition of water
b) Removal of ammonia
c) Increase of the volume of the container
d) Lowering of the reaction temperature

Quizplus · Accepted Answer

The Answer of Given the reaction below, explain how the equilibrium would be reestablished after each of the following stresses are applied. 4NH₃(g) + 3O₂(g) 2N₂(g) + 6H₂O(g) H^° = -12.0 kJ/mol a) Addition of water b) Removal of ammonia c) Increase of the volume of the container d) Lowering of the reaction temperature

Given the Reaction Below, Explain How the Equilibrium Would Be