I keep getting “Hess's law” questions wrong in Chemical Thermodynamics. What's the trap?
thinking ΔH depends on the reaction path.
The usual trap: thinking ΔH depends on the reaction path. How to avoid it: enthalpy is a state function — add steps freely. Go back to the definition — the total enthalpy change is the same no matter the route taken.
Key point
Hess's law
Common mistake
thinking ΔH depends on the reaction path.
Memory tip
enthalpy is a state function — add steps freely.
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