Question

For the reaction2 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 ____.A. spontaneous only at low temperatureB. spontaneous only at high temperatureC. spontaneous at all temperaturesD. nonspontaneous at all temperaturesE. unable to determine without more information

Answer 1

Answer:

C. spontaneous at all temperatures

Explanation:

The spontaneity of  reaction is determined by the sign of the  gibbs free energy.

A negative sign denotes that the reaction is spontaneous, positive sign means the reaction is not spontaneous.

From the question;

ΔS° = +253 J/K

ΔH° = -125 kJ/mol

ΔG = ΔH°  - TΔS°

From the data given, the condition in which we can obtain a negative value of G, is at any value of T.

For any value of T, G would always be a negative value.

This means the correct option is option C.