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This is correct. A negative value of q indicates that the system lost heat. Thus, the reaction is exothermic. A positive value of q indicates that the system gained heat. Thus, the reaction is endothermic.
Yes a +q means that the system is taking in heat therefore endothermic. a -q would mean that the system is losing heat and therefore exothermic. a +w means that the system is increasing energy by being compressed. a -w means that the system is losing energy through expansion.
If we look back at equilibrium reactions, we could predict which way a reaction must go in perspective of negative heat or positive heat energy. Exothermic processes involve the exertion of heat energy which makes the q a -q the same way -deltaH indicates an exothermic process. The same goes for endothermic process where there is a positive deltaH , indicating that heat is being absorbed, hence +q.
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