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I don't know if this is right but using the equation deltaG = deltaH - TdeltaS, I assumed that G and H would be most similar at the smallest possible values of S. This means that the correct answer is A because solids -> solids have the lowest entropy.
When entropy approaching 0, the value of TdeltaS is nearly 0, meaning Delta H is very very close to delta G, since the second term in the Gibbs Free Energy Equation goes to 0 and becomes less and less significant.
You would have to find a scenario in which enthalpy is either very large and where entropy is very small (which the above replies have covered). This is because a large enthalpy value is not likely to be skewed too much by a change in entropy. So a large negative enthalpy would correlate to a large negative delta G unless entropy is large and negative.
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