Consider the reaction below. 2 Upper N Upper H Subscript 3 (g) Baseline double headed arrow Upper N Subscript 2 (g) Baseline + 3 Upper H Subscript 2 (g). What is the most likely effect to the forward reaction if there is an increase in pressure on this reaction? The reactant surface area increases. The reaction rate decreases. The reaction is not affected at all. The reaction stops completely.

The increase in pressure of the reacting system will increase the formation of NH₃

Explanation:

The given parameters are;

2NH₃ (g) ⇄ N₂ (g) + 3H₂ (g)

The number of molecules in the reactant side of the equation = 2 molecules

The number of molecules in the product side of the equation = 1 + 3 = 4 molecules

Avogadro's law states that equal volume of all gases at a given temperature and pressure contains equal number of molecules

Therefore, given that the number of molecules of the product are twice the number of molecules of the reactant, the volume of the product is twice the volume of the reactant

If the pressure is increased, at constant temperature by Boyles law, the volume will be reduced, favoring the formation of the low volume occupying NH₃

Therefore, the reverse reaction (formation of NH₃) will preferably occur.