For the reaction 2 C₄H₁₀ (g)+ 13 O₂ (g)→ 8 CO₂ (g)+ 10 H₂O (g) ΔH° is -125 kJ/mol and ΔS° is +253 J/K ∙ mol.This reaction is ________.

Question

Quizplus · Accepted Answer

The negative value of ΔH° indicates that the reaction is exothermic (heat is released), and the positive value of ΔS° indicates that the reaction leads to an increase in the entropy of the system. A spontaneous reaction is one that occurs without requiring an external input of energy, and generally involves an increase in entropy. Given that the reaction is exothermic and increases in entropy, it will be spontaneous at all temperatures.

For the Reaction 2 C4H10 (G)+ 13 O2 (G)→ 8

For the Reaction 2 C₄H₁₀ (G)+ 13 O₂ (G)→ 8