Hydrolysis equilibrium of urotropin [closed]








**Closed.** This question is [off-topic](/help/closed-questions). It is not currently accepting answers.
 
 






---








 **Homework questions** must demonstrate some effort to understand the underlying concepts. For help asking a good homework question, see: [How do I ask homework questions on Chemistry Stack Exchange?](https://chemistry.meta.stackexchange.com/questions/141/how-do-i-ask-homework-questions-on-chemistry-stack-exchange)




Closed 7 years ago.








[Improve this question](/posts/57962/edit) 



In a test I was asked why the hydrolysis equilibrium of Urotropine (Hexamethylenetetramine) in neutral solution lies far on the side of the reactants. Well I had no idea and I'd be very glad if somebody could give me an answer on that question.




[![Urotropine hydrolysis](https://i.stack.imgur.com/qYwCC.png)](https://i.stack.imgur.com/qYwCC.png)


Small amount of acid is required for hydrolysis.
As a result ammonium salt and formaldehyde are produced.


Update:
It can be explained with enthalpy of reaction [Wiki Enthalpy of reaction](https://en.wikipedia.org/wiki/Standard_enthalpy_of_reaction). 
To calculate it, enthalpy of each reactant required. 
From wiki: ΔH(C6H12N4)=-99.2kJ/mol, ΔH(H2O)=-285.8kJ/mol, ΔH(NH3)=-45.94kJ/mol, ΔH(CH2O)=-115.9kJ/mol; 
ΔH(reaction)=6\*ΔH(CH2O)+4\*ΔH(NH3)-ΔH(C6H12N4)-6\*ΔH(H2O)=918kJ/mol; 


As ΔH(reaction) is large, positive number, a lot of heat required for this reaction, as a result, equilibrium is far on the side of the reactants.


 0