11.81

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

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

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

Ryan Fang 1D
Posts: 53
Joined: Sat Jul 22, 2017 3:00 am

11.81

A gaseous mixture consisting of 2.23 mmol N2 and 6.69 mmol H2 in a 500.-mL container was heated to 600. K and allowed to reach equilibrium. Will more ammonia be formed if that equilibrium mixture is then heated to 700. K? For N2(g) + 3 H2(g) -><- 2 NH3(g), K = 1.7 x 10^-3 at 600. K and 7.8 x 10^-5 at 700. K.

The solutions manual takes a shortcut on this question by simply comparing the equilibrium constants at the different temperatures. While I understand this answer, how would I go about solving the question with calculations instead of qualitatively?

Jingyi Li 2C
Posts: 56
Joined: Fri Sep 29, 2017 7:06 am

Re: 11.81

You could use ICE box to find the concentration of each chemical, but that requires a lot of work. Comparing the equilibrium constants is a much easier way.

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