Understanding Hess Law: Enthalpy Summation vs. Heat Change in Chemical Reactions

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Hess's Law states that the total enthalpy change in a chemical reaction is the sum of the enthalpy changes for individual steps, represented as DH = dH1 + dH2. The discussion raises a question about whether a similar summation applies to heat changes, represented as DQ = dQ1 + dQ2, and seeks clarification on its validity. The forum rules emphasize the need for users to demonstrate their understanding before receiving assistance. Additionally, there is a request for clarification on the differences between thermodynamic and kinetic stability. The conversation highlights the importance of understanding both enthalpy and heat in the context of chemical reactions.
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You people heard about hess law means that sum of all enthalpies of chemical reactions takes place but why we only call sum of all enthalpies?

1)
A----B dH1
B----C dH2 HESS LAW
DH = dH1 + dH2

2)
A----B dQ1
B----C dQ2 ?
DQ = dQ1 + dQ2
In the above representations one is associated with enthapy and another is heat
whethe second one is valid or not?if so why?
 
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Welcome to the forums syamdcs,

According to the rules of the forum, you must show your work/attempt before we can offer any assistance. Also, in future, could you please post homework questions in the appropriate forum. Thanks.
 
please i will like u to give me some major diferences btw thermodynamic and kinetic stability
 

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