Part b calculate the enthalpy change, δh∘, for the "expansion" of methane: ch4(g)→c(g)+4h(g) express your answer to one decimal place and include the appropriate units.
This equation essentially states that the standard enthalpy change of formation is equal to the sum of the standard enthalpies of formation of the products minus the sum of the standard enthalpies of formation of the reactants. and the standard enthalpy of formation values:δH fo[A] = 433 KJ/mol. δH fo[B] = -256 KJ/mol.
CH4(g) -> C(g)+4H(g)
ΔHâ/ δhâ = 1.665 MJ = 1665 KJ
