For the reaction: Fe2O3(s) + 3CO(g )  2Fe(s) + 3CO2(g ); the following values of K are known: T = 250 degrees C, K= 100 ; T = 1000 degrees C , K = .0721 At 1120 degrees C for the reaction of 2CO2(g ) ⇆ 2CO(g ) + O2(g ), k =1.4x10^-12. What equilibrium partial pressure of O2 would have to be supplied to a vessel at 1120 degrees C containing solid Fe2O3 just to prevent the formation of Fe? Show complete solution and round everything to 4 decimal places.

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For the reaction: Fe2O3(s) + 3CO(g )  2Fe(s) + 3CO2(g ); the following values of K are known: T = 250 degrees C, K= 100 ; T = 1000 degrees C , K = .0721

At 1120 degrees C for the reaction of 2CO2(g ) ⇆ 2CO(g ) + O2(g ), k =1.4x10^-12. What equilibrium partial pressure of O2 would have to be supplied to a vessel at 1120 degrees C containing solid Fe2O3 just to prevent the formation of Fe?

Show complete solution and round everything to 4 decimal places.

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