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So think of a car going down a hill and theres something at the bottom of the hill the car's going to hit. If the car breaks on its downhill approach to the object, it uses more heat than work in the process. If the car doesn't break and wildly goes straight into the object, it uses more work than heat. At the end of the day, the change in internal energy of the system is the same in both cases (since it is a state function), but the heat (q) and work (w) were different in the two scenarios since they are pathway dependent (which is why they're not state functions). I found this in a video and it helped me a bit, hope it was helpful to you to :)
Heat and work are not state functions because they depend on the path taken (like distance traveled), while enthalpy is a state function because it does not depend on what happens between the initial and final states (like elevation gain). For example, if there is a reaction in which there is no change in enthalpy (because the initial and final states are the same) but there is heat transfer involved (the same amount of heat enters and leaves the system over the course of the process).
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