Solving a Thermodynamics Problem: Finding ΔHf for OH(g) in H2O2 (g) Reaction

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Dell
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How do i solve this chem, thermodynamics problem?
find ΔHf for OH(g) if

H2O2 (g)--> 2OH(g)

ΔH(diss)=213KJ/mol

what is ΔH(diss)?? what is 'diss'

someone told me The ΔH(diss)=213KJ/mol is equal to twice the ΔHf of OH. but i doont know how they got to this, also it seems a bit too simple for a qestion if all i need to do is divide by 2,
so how would i solve this?
 
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Your [tex]\Delta H(diss)[/tex] is your enthalpy of reaction. Remember that the enthalpy of reaction equals: Enthalpy of formation of products - Enthalpy of formation of reactants. Replace your data (you will need to look for H2O2 enthalpy of formation on a table) there and solve for [tex]\Delta H(OH)[/tex].