🤓 Based on our data, we think this question is relevant for Professor Kuebler's class at UCF.
We can rely on the change in entropy-based on a phase change to determine the given reaction's spontaneity. It should have a positive sign (i.e. reaction favors the formation of a product with higher disorder/entropy).
The reaction is:
2 CO(g) + O2(g) → 2 CO2(g) ΔH˚rxn = –556.0 kJ
Without doing any calculations, determine the sign of ΔSsys and ΔSsurr for each of the chemical reactions below. In addition, predict under what temperatures (all temperatures, low temperatures, or high temperatures), if any, the reaction will be spontaneous.
2 CO(g) + O2(g) → 2 CO2(g), ΔH˚rxn = –556.0 kJ