## example 9.16 [ENDORSED]

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

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

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

Liam Maxwell 2E
Posts: 53
Joined: Fri Sep 29, 2017 7:07 am

### example 9.16

the question asks you to estimate the temperature at which it is thermodynamically possible for a reaction to occur. In the explanation it says when temp is increased there is a point where T= standardH/standardS. However in order for this to be true following the equation StandardG=StandardH-TstandardS wouldn't that mean G is 0 and therefore the equation is at equilibrium and therefore the reaction won't have a net occurence?

Chem_Mod
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### Re: example 9.16  [ENDORSED]

Solving for the point at which $\Delta G=0$ is indeed the condition for equilibrium. To be precise, you are solving for this point so you can describe the inequality. It is the > or < that we are interested in. However, to know this, we must first determine the equilibrium temperature as you wrote.