N2(g) + 3H2(g) ⇄ 2NH3(g) ΔH = -92kJmol-1 Consider the chemical reaction for the manufacture of ammonia in the Haber process. The ΔH value shows that the reaction is exothermic. What would be the effect on the position of equilibrium if you increased the pressure? All BUT ONE choice applies. A) More ammonia would be formed. B) The position of equilibrium would move to the right. C) The reaction would change from exothermic to endothermic. D) According to Le Chatelier, if you increase the pressure, the system will respond by reducing it again.