N₂(g) + 3H₂(g) ⇌ 2 NH₃ (g); ΔHrxn = -92.4 kJ, meaning the reaction is exothermic. Given the aforementioned details, how will the equilibrium of the system be affected if (a) more N₂ will be added, (b) decrease in temperature, and (c) increase in pressure?
A. Increase in pressure will favor the forward reaction
B. Increase in pressure will favor the reverse reaction
C. Adding more N₂ will favor the reverse reaction
D. Decrease in temperature will favor the forward reaction
E. Decrease in temperature will favor the reverse reaction
F. Adding more N₂ will favor the forward reaction
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