Question

Use the reaction data in the table below to select the answer choice that best describes this reaction.



Reaction Enthalpy Change
345.7 kJ/mol
Reaction Entropy Change
-25. 3 J/molK



This reaction is never spontaneous.


This reaction is spontaneous at all temperatures.


This reaction is spontaneous at low temperatures.


This reaction is spontaneous at high temperatures

Answer 1

Answer: This reaction is never spontaneous

Explanation:

According to Gibbs equation:

$\Delta G=\Delta H-T\Delta S$

$\Delta G$ = Gibb's free energy change

$\Delta H$ = enthalpy change

T = temperature

$\Delta S$ = entropy change

A reaction becomes spontaneous when $\Delta G$ = Gibb's free energy change is negative.

$\Delta G=+ve-T(-ve)$

$\Delta G=+ve+ve$

$\Delta G=+ve$

Thus this reaction is never spontaneous