Given the bond energies N ≡ N, H − H and N − H bonds are 945,436 and 391 kJ mole−1 respectively, the enthalpy of the following reaction N2(g) + 3H2(g) → 2NH3(g) is
-93 kJ
N ≡ N + 3H −H → 2N|H|H−H
945 +3 x 436 2 × (3 × 391) = 2346
Energy absorbed Energy released
Net. Energy released = 2346 − 2253 = 93 kJ
i.e., ΔH = −93kJ