Question

mmonia, NH3, is used in numerous industrial processes, including the production of pharmaceuticals such as sulfonamide and antimalarials and vitamins such as the B vitamins. The equilibrium equation for the synthesis of ammonia (sometimes known as the Haber process) is N2(g) + 3H2(g) ↔ 2NH3(g) What would happen to the rate of the forward reaction if the concentration of nitrogen were decreased? The reaction rate would

Answer 1

Answer:

An addition of nitrogen gas will cause the forward the reaction to be favored, increasing the rate of the reaction.  This question can be explained using Le Chatelier's principle

Explanation:

Le Châtelier’s Principle states that if a dynamic system is subjected to change in external conditions, the equilibrium will shift to minimize the effects of that conditioning. External conditions are factors that cause the rate of the forward or reverse reaction to change; so if the system encounters any changes in pressure, temperature, or concentration of products or reactants, the equilibrium shifts in the opposite direction to offset the change.

If the concentration of an substance in a system is increased, the system will favour the reaction which removes that substance.

Therefore, an addition of nitrogen gas will cause the forward the reaction to be favoured, since that is the reaction that would echaust the N2 gas. The forward reaction speeds up temporarily as a result of the addition of a reactant..