Chapter 4, Problem 4J.5BST

Interpretation Introduction

Interpretation:

The value of standard Gibb’s free energy change for equation ${\text{6CO}}_{\text{2}}\left(\text{g}\right)+{\text{12H}}_{\text{2}}\text{O}\left(\text{l}\right)\to {\text{C}}_{\text{6}}{\text{H}}_{\text{12}}{\text{O}}_{\text{6}}\left(\text{s}\right)+{\text{6O}}_{\text{2}}\left(\text{g}\right)$ has to be calculated.

Concept Interpretation:

The quantity that enables one to predict the reaction’s spontaneity is Gibbs free energy $\left(\Delta G\right)$ and it changes with a change in temperature. The value of $\Delta G$ can be deduced by the equation,

  $\Delta G_{\text{rxn}}^{\text{ο}}={\displaystyle \sum m\cdot \Delta G_{\text{f}}^{\text{ο}}}\left(\text{products}\right)-{\displaystyle \sum n\cdot \Delta G_{\text{f}}^{\text{ο}}}\left(\text{reactants}\right)$

The values of Gibb’s free energy can determine the stability of the compound.  The negative value determines the thermodynamically stable compound and positive value determines thermally unstable compound.