If the bond energies of H - H , B r - B r , a n d H - B r a r e 433 , 192 a n d 364 k J m o l - 1 respectively, the ∆ H o for the reaction H 2 g + B r 2 g → 2 H B r g is

Question

If the bond energies of H - H , B r - B r , a n d H - B r a r e 433 , 192 a n d 364 k J m o l - 1 respectively, the ∆ H o for the reaction H 2 g + B r 2 g → 2 H B r g is, - 261 k J, + 103 k J, + 261 k J, - 103 k J

MARKS App · Accepted Answer

H 2 g + B r 2 g → 2 H B r g Enthalpy change for this reaction will equal to the difference in the energy consumed for breaking bonds of reactants and energy released when bonds of products are made Enthalpy = Sum of bond energies broken - sum of bond energies formed ∆ H o = B E r e a c t a n t - B E p r o d u c t = 433 + 192 - 2 × 364 = 625 - 728 = - 103 k J

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