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JIPMER Jipmer Medical Solved Paper-1995

  • question_answer
    Consider the reactions: \[C(s)+2{{H}_{2}}(g)\xrightarrow{{}}C{{H}_{4}}(g);\]    \[\Delta H=-x\,kcal\] \[C(g)+4H(g)\xrightarrow{{}}C{{H}_{4}}(g);\]    \[\Delta H=-\,y\,kcal\] \[C{{H}_{4}}(g)\xrightarrow{{}}C{{H}_{3}}(g)+H(g);\]  \[\Delta H=+\,z\,kcal\] The bond energy of C?H bond is:

    A)  \[\text{y}\,\text{kcal}\,\text{mo}{{\text{l}}^{-1}}\]    

    B)                         \[z\,\text{kcal}\,\text{mo}{{\text{l}}^{-1}}\]                     

    C)         \[\frac{x}{4}\,\text{kcal}\,\text{mo}{{\text{l}}^{-1}}\]                  

    D)         \[\frac{y}{2}\,\text{kcal}\,\text{mo}{{\text{l}}^{-1}}\]

    Correct Answer: B

    Solution :

    \[C{{H}_{4}}(g)\xrightarrow{{}}C{{H}_{3}}(g)+H(g);\]\[\Delta H=+z\,kcal\] In this reaction, one C?H bond is breaking hence, \[\Delta H\] represent the bond dissociation energy of C?H bond. Hence C?H bond energy is z kcal.


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