# As glucose is oxidized to carbon dioxide, does the level of entropy increase?

Jun 12, 2017

What do you think..........?

#### Explanation:

Consider the stoichiometric equation that represents such oxidation......

${C}_{6} {H}_{12} {O}_{6} \left(a q\right) + 6 {O}_{2} \left(g\right) \rightarrow 6 C {O}_{2} \left(g\right) \uparrow + 6 {H}_{2} O \left(l\right)$

The reaction is certainly favoured by enthalpy in that you making the stable carbon dioxide and water molecules.......

The reaction is also favoured by entropy in that a linear triatom, the $C {O}_{2}$ certainly has more statistical probability for disorder than a diatom. Entropy increases, and you should use the tables of standard entropy that you will find in your text to calculate the $\Delta {S}^{\circ}$ of the given reaction (you can ignore the entropies of the solid and the liquid, $S {\text{_"gas}}^{\circ}$ will dwarf these.......In any case in the reaction as written you've got 12 moles of product, and 7 moles of reactant; what do these data suggest with regard to entropy?