Question

formation of glucose
thermodynamic favorability
consider what you know or can predict
regarding the enthalpy, entropy, and free
energy of the reaction below.
\\(\delta g_{\text{rxn}} = +870\\ \text{kj}\\)
\\(6\text{co}_2(\text{g}) + 6\text{h}_2\text{o}(\text{g}) \
ightarrow \text{c}_6\text{h}_{12}\text{o}_6(\text{s}) + 6\text{o}_2(\text{g})\\)
which choice correctly describes the
thermodynamic favorability of the
reaction?
the reaction is thermodynamically favorable at
high temperatures.
the reaction is always thermodynamically
favorable.
the reaction is never thermodynamically
favorable.
the reaction is thermodynamically favorable at low
temperatures.

Explanation:

To determine the thermodynamic favorability of a reaction, we use the Gibbs free energy change ($\Delta G_{\text{rxn}}$). A reaction is thermodynamically favorable (spontaneous) when $\Delta G_{\text{rxn}} < 0$. If $\Delta G_{\text{rxn}} > 0$, the reaction is non - spontaneous (not thermodynamically favorable) under the given conditions. Here, $\Delta G_{\text{rxn}} = + 870\space kJ$, which is a positive value. This means that regardless of temperature (since the sign of $\Delta G$ is already positive), the reaction will not be thermodynamically favorable.

Answer:

The reaction is never thermodynamically favorable.