Given the reaction at equilibrium n2(g) + 3h2(g) ↔ 2nh3(g) increasing the concentration of N2(g) will increase the forward reaction rate due to 1. A decrease in the number of effective collisions

For the given reaction an increase in the forward reaction rate due to increase in the number of effective collisions.

Explanation:

According to the rate law, rate of a reaction depends on the concentration of its reactants. So, more is the number of reactants then more will be the number of collisions taking place.

As a result, more will be the amount of product formed. For example, in the reaction an increase in means an increase in the number of reactants.

Hence, more is the number of collisions taking place leading to more amount of formation of products.

Thus, we can conclude that for the given reaction an increase in the forward reaction rate due to increase in the number of effective collisions.