Your logic is hard to follow, so getting wrong results isn't so surprising. For instance, 47.6kJ is the heat for a reaction, not for H2, so doubling it won't suffice to inject in the unknown line.
More fundamentally, there is no ΔH associated with a species or a group of species as you try to write in the text. ΔH is associated with a transformation, here a chemical reaction, as in the title. So much that, when tables give "enthalpies of formation", they tell explicitly what the reference is - most often, the transformation is the formation of the compound, starting from the elements in their normal state (molecules of solid, liquid, gas), and often the heat is given for elements and compounds at 298K.
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-47.6kJ is the heat of formation of ethane from the elements
-1755.6kJ is its heat of combustion
From both, you can extract the heat of formation of the combustion products together.
-221.3kJ is the heat of formation of CO2, so you also deduce the heat of formation of H2O.
Reversing and multiplying the heat of formation of H2O, you get the heat of the unknown transformation.