The reaction N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g) has the following values at 298 K: K_p = 6.2×10⁵  and ΔH° = –92.2 kJ. Consider the following changes below which will result in an increase in the partial pressure of NH₃ at equilibrium. Which of the changes will result in the highest increase in the partial pressure of NH₃? Justify your answer. 

I. Adding 0.20 mol of N₂

III. Adding 0.20 mol of H₂

III. Lowering the temperature to 250 K

A. Adding 0.20 mol of N₂ will result in the highest increase in partial pressure of NH₃ because it will produce a greater amount of NH₃.

B. Adding 0.20 mol of H₂ will result in the highest increase in partial pressure of NH₃ because it is the limiting reactant.

C. Lowering the temperature to 250 K will result in the highest increase in partial pressure of NH₃ because it will shift the equilibrium reaction to the right.

D. All of the above will result in the same increase in the partial pressure of NH₃.