## delta G formation

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

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

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

Emily Glaser 1F
Posts: 156
Joined: Thu Jul 27, 2017 3:01 am

### delta G formation

What was stated in class about H2(g) --> H2(g) and its delta G of formation/entropy?

I know for this reaction, delta H of formation would be zero.
Is delta G of formation zero?
Does that mean delta S is zero too?

Vasiliki G Dis1C
Posts: 53
Joined: Fri Sep 29, 2017 7:04 am

### Re: delta G formation

The ΔGf would also be 0 because there is no change between the reactants and products, and H2 is in its most stable form. If you know ΔHf is 0, and ΔGf is 0, then you can also conclude that ΔSf would also be 0 (using ΔG=ΔH-TΔS). Hope this helps!

Katie Lam 1B
Posts: 52
Joined: Fri Sep 29, 2017 7:06 am

### Re: delta G formation

Since the hydrogen gas is still the same substance, the entropy will not change.