N2 (g)+3 H2 (g)⇌2 NH3 (g) Figure 1: Ammonia gas formation and equilibrium What would most likely happen if a scientist decreased the volume of the container in which the Does reaction occur?
Answers
Answer:
The equilibrium constant for the reaction N2(g) + 3H2(g) = 2NH3(@) at 500 K is 100.
Answer:
On decreasing the volume of the container, more NH₃ will be produced.
Explanation:
The pressure will increase when the volume is decreased. According to the Le-Chatlier principle, the equilibrium will shift to the side accompanied by a decrease in pressure or a decrease in the number of gaseous moles.
n(products) > n(reactants) →the reaction will go in the backward direction
n(reactants) > n(products) →the reaction will go in the forward direction
n(products) = n(reactants) →the reaction will not be affected by the change in volume.
The reaction is given below.
N₂(g) + 3H₂(g) ⇌ 2NH₃(g)
In this case, the number of moles on the product side(2 moles) is less than the number of moles on the reactant side(3 + 1 = 4 moles). Thus, the equilibrium will shift in the forward direction and will favour the formation of ammonia.