## 4J7

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

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

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

Samantha Hoegl Roy 2C
Posts: 81
Joined: Fri Sep 28, 2018 12:15 am

### 4J7

For this question we are asked to calculate the stanfard reaction entropy, enthalpy and Gibbs free energy

A) 2 H2O2 —> 2 H2O + O2
Why do they nt divide the result by 2? I thought that for standard G,S and H, it was all for 1 mol of product and sinxe there are 2 mol of H2O2 I am a bit confused

Elisa Bass 4L
Posts: 61
Joined: Fri Sep 28, 2018 12:23 am

### Re: 4J7

∆G, ∆S, and ∆H are all expressed in terms of one mole of reaction. You already account for the number of moles involved when you used the S°m, ∆H°f, and ∆G°f for each reactant/product, so the result you calculate is in terms of the reaction as a whole.