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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.

Respuesta :

Answer:

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

Explanation:

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

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

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

To find ΔG for reaction :

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

By using Hess's law:

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

[tex]\Delta G =\Delta G_1-\Delta G_2-\Delta G_3[/tex]

[tex]=13.2 kJ/mol -(-28.9 kJ/mol)-(5.80 kJ/mol)=36.3 kJ/mol[/tex]

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

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