## 5J.15

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

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

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

AlyssaYeh_1B
Posts: 100
Joined: Sat Aug 17, 2019 12:16 am

### 5J.15

This question asks us to calculate the equilibrium constants for two reactions at 25C and 150C. Can someone walk me through the problem? I'm unsure of where to start. I assume we need to calculate delta G, but which equation would we use to calculate K? These are the reactions:

(a) NH4Cl(s) <--> NH3(g) + HCl(g)
(b) H2(g) + D2O(l) <--> D2(g) + H2O(l)

Parker Smith
Posts: 102
Joined: Thu Jul 25, 2019 12:15 am

### Re: 5J.15

Once you find delta G, you can use the delta G= delta G0 + RTln(Q) equation, or more specifically, the delta G0= -RTln(K)

Rebekah Alfred 1J
Posts: 102
Joined: Thu Jul 11, 2019 12:15 am
Been upvoted: 1 time

### Re: 5J.15

To calculate K, you need to manipulate the first equation in this image to the last equation: