Reactions and Themodynamics Related Question

[predentalgirl1]

1.) (a) Give the reaction, with molecular structures, of 2-propanol with KMnO4 and 1-pentanol with KMnO4 and calculate the differences in the average bond energies of the reactants and products (ignore KMnO4 and any other side reactions in the calculations).
Answer:-
the reaction, with molecular structures, of 2-propanol with KMnO4,is

5CH3CHOHCH3 + 2KMnO4 + 6H+ → 5CH3COCH3 + 2Mn2 + + 8H2 O



bond energy of reactants= C – C is 3 x 80 = 240
C – H is 7 x 98=686
C – O is 1 x 78=78
O – H is 1 x 110=110
The total bond energy of reactants = 240+686+78+110= 1114kcal/mole

bond energy of products= C – C is 3 x 80 = 240
C – H is 6 x 98=588
C= O is 1 x 187=187
The total bond energy of products = 240+588+187= 1015kcal/mole
the differences in the average bond energies of the reactants and products,
= 1114-1015= -99kcal/mole


(THIS WILL NOT POST RIGHT FOR SOME REASON...)

H H H H H H H H H
****|***|***|***|***|**************KMnO4********| | | |
*********H -C-C-C-C-C-OH***** ------->**** H-C-C-C-C-C=O
***************|****|****|***|**|******************************** **| | | | |****************
H H H HH H H H H H


bond energy of reactants= C – C is 4 x 80 = 320
C – H is 11 x 98=1078
C – O is 1 x 78=78
O – H is 1 x 110=110
The total bond energy of reactants = 320+1078+78+110= 1586kcal/mole

bond energy of products= C – C is 4 x 80 = 320
C – H is 10 x 98=980
C= O is 1 x 187=187
The total bond energy of products = 320+980+187= 1487kcal/mole
the differences in the average bond energies of the reactants and products,
= 1586-1487= -99kcal/mole





(b) From your calculations does it appear that formation of the ketone or the carboxylate salt is more thermodynamically favored? Why?
Answer:-

From the calculations it is seen that both the reactions are thermodynamically favaoured. Since, the bond energy of the products is less than that of reactants.


Is this correct guys?

 

[nate808]

Yes, your calculations and reasoning are correct. The formation of both the ketone and the carboxylate salt is thermodynamically favored, as the bond energies of the products are lower than those of the reactants.

 

[Blueshift5]

Yes, your calculations and conclusion are correct. The formation of both the ketone and the carboxylate salt is thermodynamically favored, as the bond energy of the products is lower than that of the reactants. This indicates that the products are more stable than the reactants, making the reactions spontaneous and thermodynamically favorable.