Question

Why is it possible for the ∆G values in Table 15-1 to differ from the ∆G°ˈ values?

Short answer

The values of cellular reactant and product vary at different temperature and change in enthalpy.

$∆\mathrm{G}=∆\mathrm{G}°+\mathrm{RTln}\left(\begin{array}{c}\left[\mathrm{Product}\right]\\ \left[\mathrm{Reactant}\right]\end{array}\right)$

Step-by-step solution

Introduction

Gibb's free energy describes how much of a system's total energy is used in a chemical reaction. ∆G represents the shift in free energy. ∆G is anticipated by temperature and enthalpy changes. The typical free energy change is symbolised by "∆G".

Reason for the ∆G values differ from ∆G°ˈ

Glycolysis is a continuous process in most tissues under steady-state circumstances, while the glycolysis flow changes to fulfill the demands of the organism. Each reaction in the route is related to the standard free energy changes (∆G°ˈ) and the real physiological free energy changes (∆G). Because of the link between (∆G°ˈ) and (∆G), which is expressed by the following equation:

$∆G=∆G°+RT\ln \left(\begin{array}{c}\left[Product\right]\\ \left[Reac\tan t\right]\end{array}\right)$

Interpretation

Thus, various reactions proceed in animal tissues; as a result, the values of the cellular reactant and product alter with temperature and enthalpy, and they are not equal in their standard states.