Question

formation of butane from carbon dioxide and water
thermodynamic favorability
consider what you know or can predict regarding the enthalpy, entropy, and free energy of the reaction below.
\\(\delta g_{rxn} = 5408kj\\)
\\(8co_2(g) + 10h_2o(g) \
ightarrow 2c_4h_{10}(g) + 13o_2(g)\\)
which choice correctly describes the thermodynamic favorability of the reaction?
the reaction is always thermodynamically favorable.
the reaction is thermodynamically favorable at high temperatures.
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, $\Delta G_{\text{rxn}} = 5408\space kJ$, which is a positive value. So, the reaction is never thermodynamically favorable.

Answer:

The reaction is never thermodynamically favorable.