The atomisation enthalpy of CH_4 is 1660 kJ | vedclass

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(B) The atomisation enthalpy of $CH_4$ is $1660 \ kJ \ mol^{-1}$.$CH_{4(g)} \longrightarrow C_{(g)} + 4H_{(g)} ; \Delta_a H = 1660 \ kJ \ mol^{-1}$Mea

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$325 \ kJ \ mol^{-1}$

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(B) The atomisation enthalpy of $CH_4$ is $1660 \ kJ \ mol^{-1}$.$CH_{4(g)} \longrightarrow C_{(g)} + 4H_{(g)} ; \Delta_a H = 1660 \ kJ \ mol^{-1}$Mean $C-H$ bond enthalpy $= \frac{1660}{4} = 415 \ kJ \ mol^{-1}$.Let the bond enthalpies of the four $C-H$ bonds be $E_1, E_2, E_3, E_4$.Given: $E_1 = 415 + 15 = 430 \ kJ \ mol^{-1}$,$E_2 = 415 + 30 = 445 \ kJ \ mol^{-1}$,$E_3 = 415 + 45 = 460 \ kJ \ mol^{-1}$.The sum of all bond enthalpies equals the atomisation enthalpy:$E_1 + E_2 + E_3 + E_4 = 1660$$430 + 445 + 460 + E_4 = 1660$$1335 + E_4 = 1660$$E_4 = 1660 - 1335 = 325 \ kJ \ mol^{-1}$.

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