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(a) Compute the rate constant for the oxidation of Fe2+ below in a water sample that is open to the atmosphere given that half of the Fe2+ is consumed after 23 seconds at 25 degrees C. Presume first order kinetics with respect to Fe2+ Fe2+(aq) + O2(aq) <--> Fe3+ (aq) + O2(-) (aq)

(b) Compute the activation energy for the oxidation of Fe2+ if half of the Fe2+ is consumed after 15 seconds.

(c) For the same water utilized in part an above that isn't open to the atmosphere, half of the Fe2+ is consumed after 45 seconds at 25 degrees C?

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