A chiral C5H10O ether reacts with excess hot HI to give a C5H10I2 product. When this product is treated with KOH, 1,3-pentadiene
1 answer:
Answer:
See answer and picture below
Explanation:
In this case, the key to get an idea of how is the starting ether is with the final product and the empirical formula of the ether.
First, the empirical formula of the ether gives us information of the structure of the ether. This ether could be either an alkene, alkane or cycloalkane.
Alkane cannot be because alkane's formula is CnH(2n+2), so it's either an alkene or cycloalcane (CnH2n).
However, as we can see, it reacts with HI in excess, so, it cannot be an alkene because in this case the acid will react with the double bond of the ether too forming another product. This discart the fact that the ether has a double bond. So it has to be a cycloalkane.
As the innitial structure it's an ether, it should be either a cyclohexane or cyclopentane with a methyl group attached. So, how can we know which of these structures is? well, we can actually do the reaction with both reactants and see which match. In the attached picture you have the answer.
Hope this helps.
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Answer : The enthalpy change for the reaction is, 201.9 kJ
Explanation :
According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.
According to this law, the chemical equation can be treated as ordinary algebraic expression and can be added or subtracted to yield the required equation. That means the enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.
The balanced reaction of will be,
The intermediate balanced chemical reaction will be,
(1)
(2)
(3)
(4)
Now we will multiply the reaction 1 by 2, revere the reaction 2, reverse and half the reaction 3 and 4 then adding all the equations, we get :
(1)
(2)
(3)
(4)
The expression for enthalpy of the reaction will be,
Therefore, the enthalpy change for the reaction is, 201.9 kJ