Question

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.

Answer 1

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

Step-by-step explanation:

`{\rm A \rightleftharpoons B}, \Delta G_1 = 13.2 kJ/mol`...[1]

`{\rm B \rightleftharpoons C}, \Delta G_2 = -28.9 kJ/mol`...[2]

`{\rm C \rightleftharpoons D},\Delta G_3 = 5.80 kJ/mol`...[3]

To find ΔG for reaction :

`{\rm A \rightleftharpoons D},\Delta G = ?`...[4]

By using Hess's law:

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

`\Delta G =\Delta G_1-\Delta G_2-\Delta G_3`

`=13.2 kJ/mol -(-28.9 kJ/mol)-(5.80 kJ/mol)=36.3 kJ/mol`

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