Consider the reaction below. 2NH3g+N2g+3H2g 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 position of the equilibrium will shift towards the products. Thus, when pressure is increased the rate of the forward reaction is increased.

Explanation:

For the reversible response:  

                         N2 (g) + 3H2  (g) ⇌ 2NH3  (g) + heat.  

The equilibrium moves forward way  by expanding pressure and diminishing temperature.   As indicated by the Le-Chatalier principle when equilibrium is disturbed by a change, the system will try to nullify the impact of change to restore the balance.   Subsequently, when pressure is expanded, the equilibrium will move toward a path in which there is a decrease in the number of moles of vaporous substances. This will invalidate the impact of expanded pressure.   This occurs the forward way.   Also for an exothermic response, when the temperature is diminished, the equilibrium shifts in forwarding direction.

Noble gases is far right