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Calculate the standard enthalpy of formation of methane, CH4 (g), using a C-H bond enthaply of 413 kJ mol-1 and the atomization enthalpies of 716.682 and 217.96 kJ mol-1, respectively for C and H.

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Keith Leannon
Keith LeannonLv2
28 Sep 2019

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Related questions

given that the average bond energies for C-H and C-Br bonds are 413 kj/mol and 276 kj/mol respectively, calculating the heat of atomization (breaking into atoms) of bromoform CHBr3


For the reaction: H2(g)+C2H4(g)-->C2H6(g)

Bond & Bond Enthalpy

H-H 436.4 kJ/mole

C-H 414 kJ/mol

C-C 347 kJ/mol

C=C 620 kJ/mol

Substance & delta Hf

H2 0

C2H4 52.3

C2H6 -84.7

(a) estimate the enthalpy of reaction, using the bond enthalpy values from the table in kJ/mol

(b) Calculate the enthalpy of reaction, using standard enthalpies of formation

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