## +DeltaG

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

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

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

Patrick Wilson 2B
Posts: 22
Joined: Wed Sep 21, 2016 3:00 pm

### +DeltaG

If Delta G is positive than the process is not spontaneous, but does this mean it wants to go back to equilibrium and the reverse reaction starts or does it just stay where it is ?

Jonathan Sarquiz 3F
Posts: 32
Joined: Fri Jul 15, 2016 3:00 am

### Re: +DeltaG

Using the example in the course reader of Br2 liquid $\rightarrow$ Br2 gas, we determined that the boiling point was 333K.

If T < 333 K, then the reaction is non spontaneous. This means that if you have a beaker of liquid bromine and you walk into a room that is at 300K, it will stay as liquid bromine. But, if you have a beaker of bromine gas and walk into a room that is at 300K, the gas will turn into a liquid by itself (spontaneous reaction).

If T > 333 K, then the reaction is spontaneous. This means that if you have a beaker of bromine gas and you walk into a room that is at 350K, it will stay as bromine gas. But, if you have a beaker of liquid bromine and walk into a room that is at 350K, the liquid will turn into gas by itself (spontaneous reaction).