Question

Consider these hypothetical chemical reactions:

A⇌B,ΔG= 14.3 kJ/mol
B⇌C,ΔG= -30.2 kJ/mol
C⇌D,ΔG= 6.20 kJ/mol

What is the free energy, ΔG, for the overall reaction, A⇌D?

Answer 1

The overall free energy change (ΔG) for the reaction A⇌D is calculated by summing up the individual ΔG values for each step of the path, resulting in a total ΔG of -9.7 kJ/mol.

Step-by-step explanation:

To calculate the free energy change (ΔG) for the overall reaction from A to D, we simply add the free energy changes of the individual steps in the reaction pathway.

• The free energy change for A to B is 14.3 kJ/mol.
• The free energy change for B to C is -30.2 kJ/mol.
• The free energy change for C to D is 6.20 kJ/mol.

By adding these values together, we can find the overall free energy change:

14.3 kJ/mol (A to B) - 30.2 kJ/mol (B to C) + 6.20 kJ/mol (C to D) = -9.7 kJ/mol (A to D)

Therefore, the ΔG for the overall reaction A⇌D is -9.7 kJ/mol.