## Example 19.14 (6th edition)

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

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

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

Alondra Olmos 4C
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### Example 19.14 (6th edition)

In this example in the textbook the first step of solving the problem was finding the standard enthalpy of formation in which they multiplied by the number of moles. However, when they applied the value they found into Gibb’s equation, they multiplied by the number of miles again. Why is that?

Chem_Mod
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### Re: Example 19.14 (6th edition)

Can you clarify what homework question this is regarding and perhaps write out the problem? 19.14 is not one of the homework problems you are responsible for, nor is that chapter related to Gibb's Free Energy.