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All you need to know about enthalpy so far is that negative enthalpy means exothermic and a positive enthalpy means endothermic. Therefore, heating up an endothermic reaction causes equilibrium to favor products, and cooling an exothermic reaction causes equilibrium to favor products too.
For right now, we only need to use delta H to determine is a reaction is endothermic or exothermic. If delta H is positive, the reaction is endothermic. If delta H is negative, the reaction is exothermic.
I think last class Dr. Lavelle mentioned that there are three(?) ways of calculating delta H and that he'd teach us how to do it (if not now then eventually). However, for now it is important to know that positive delta H means that the reaction is endothermic and that heating the system will shift the reaction forward (towards the products), and that negative delta H means that the reaction is exothermic and that heating the system will shift the reaction backward (towards the reactants).
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