MHT CET Chemistry question
Energies required to break the individual C-H bonds in each successive step differ
\mathrm{CH_4(g) \to CH_3(g) + H(g);\ \Delta_{bond}H^{\ominus} = 427\ kJ\,mol^{-1}}
\mathrm{CH_3(g) \to CH_2(g) + H(g);\ \Delta_{bond}H^{\ominus} = 439\ kJ\,mol^{-1}}
\mathrm{CH_2(g) \to CH(g) + H(g);\ \Delta_{bond}H^{\ominus} = 452\ kJ\,mol^{-1}}
Therefore,
In such cases we use
Answer: (C)
Solution
Since the four successive CH dissociation energies differ, the average kJ mol is used and is called the mean (average) bond enthalpy; (a)
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