Fe3O4(s) + 4H2(g)3Fe(s) + 4H2O(g) H° = 151.2 kJ and S° = 169.4 J/K The standar

Chemistry
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Fe3O4(s) + 4H2(g)3Fe(s) + 4H2O(g)


H° = 151.2 kJ and S° = 169.4 J/K

The standard free energy change for the reaction of 1.89 moles of Fe3O4(s) at 346K, 1 atm would be  kJ.

This reaction is (reactant, product)  favored under standard conditions at 346 K.

Assume that H° and S° are independent of temperature.
Jun 2nd, 2015

Please let me know if you need any clarification. I'm always happy to answer your questions.

delta G = 151.2 - (346 * 169.4) = -58461.2 J

                                                  = -58.46 kJ

Product favoured

Please let me know if you have any questions and best me if you are satisfactory.

Jun 3rd, 2015

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