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If DeltaG = - 177 K cal for (1) 2 Fe(s) ...

If `DeltaG = - 177 K cal` for (1) `2 Fe(s) + (3)/(2)O_(2)(g) rarr Fe_(2)O_(3)(s)` and
`DeltaG = - 19 K cal` for (2) `4 Fe_(2)O_(3)(s) + Fe(s) rarr 3 Fe_(3)O_(4) (s)`
What is the Gibbs free energy of formation of `Fe_(3)O_(4)` ?

A

`+ 229.6 (kcal)/(mol)`

B

`- 242.3 (kcal)/(mol)`

C

`- 727 (kcal)/(mol)`

D

`- 229.6 (kcal)/(mol)`

Text Solution

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