Consider these hypothetical chemicalreactions:
{\rm a \rightleftharpoons b}, \quad\delta g = 13.2 kj/mol
{\rm b \rightleftharpoons c}, \quad\delta g = -28.9 kj/mol
{\rm c \rightleftharpoons d},\quad \delta g = 5.80 kj/mol
what is the free energy, delta g, for the overall reaction, \rm a \rightleftharpoons d ?
express your answer numerically inkilojoules per mole.

The value of free enrage that is ΔG for the overall reaction is  36.3 kJ/mol.

Explanation:

...[1]

...[2]

...[3]

To find ΔG for reaction :

...[4]

By using Hess's law:

[1] - [2] - [3] = [4]

The value of free enrage that is ΔG for the overall reaction is  36.3 kJ/mol.

hi,

the answer is d.indefinite shape but definite volume, let go oogle u out

hope this !

thats how its supposed to be