## 4J.1

$\Delta G^{\circ}= \Delta H^{\circ} - T \Delta S^{\circ}$

$\Delta G^{\circ}= -RT\ln K$

$\Delta G^{\circ}= \sum \Delta G_{f}^{\circ}(products) - \sum \Delta G_{f}^{\circ}(reactants)$

Amy Luu 2G
Posts: 105
Joined: Wed Sep 18, 2019 12:19 am

### 4J.1

Why are so many exothermic reactions spontaneous?
Looking at the equation $\Delta$G = $\Delta$H - T$\Delta$S, in order for a reaction to be spontaneous, $\Delta$G must be negative. What does an exothermic reaction tell us about the enthalpy change or entropy change?

JohnWalkiewicz2J
Posts: 103
Joined: Thu Jul 11, 2019 12:17 am
Been upvoted: 1 time

### Re: 4J.1

If a reaction is exothermic than ΔH will be negative. If ΔH is negative and the exothermic reaction leads to a increase in entropy of the system(+ΔS) than ΔG will be negative and the reaction will occur spontaneously.