If the bond energies of H − H , Br − Br , and H − Br are 433,192 and 364 kJ / mol − 1 respectively, the Δ H ∘ for the reaction H 2 ( g ) + Br 2 ( g ) → 2 HBr ( g ) is:NEET 2004

Question

If the bond energies of H − H , Br − Br , and H − Br are 433,192 and 364 kJ / mol − 1 respectively, the Δ H ∘ for the reaction H 2 ( g ) ​ + Br 2 ( g ) ​ → 2 HBr ( g ) ​ is:NEET 2004

TestHub · Accepted Answer

H − H + Br − Br → 2 H − Br 433 + 192 = 625 ​ 2 = 728 ​ × 364 Energy absorbed Energy released Net energy released = Σ H R ​ − Σ H p ​ = 625 − 728 = − 103 kJ . Related Theory Fluorine has high bond energy because it is smallest among these molecules so it is tightly bonded to other atoms due to greater nuclear charge.

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