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JEE Main & Advanced Chemistry Thermodynamics / रासायनिक उष्मागतिकी Question Bank Bond energy

  • question_answer
    If the bond energies of \[H-H\], \[Br-Br\] and \[HBr\] are 433, 192 and 364 \[kJ\,mo{{l}^{-1}}\] respectively, the \[\Delta {{H}^{o}}\] for the reaction, \[{{H}_{2}}(g)+B{{r}_{2}}(g)\to 2HBr(g)\] is [CBSE PMT 2004]

    A)                 + 261 kJ

    B)                 ? 103 kJ

    C)                 ? 261 kJ

    D)                 + 103 kJ

    Correct Answer: B

    Solution :

               \[H-H+Br-Br\to 2H-Br\]            \[433+192\]           \[2\times 364\]             625                     728            Energy absorbed = Energy released            Net energy released \[=728-625=103\,kJ\]                                 i.e., \[=\Delta H=-103\,KJ\]


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