question that requires high experience in inorganic chemistry?

Your equation is well known and has applications as an auxillary supply of O2 in mines, submarines and space vehicles.

N. N. Greenwood, A. Earnshaw, Chemistry of the Elements 2nd ed. (1997) p 74

The Cu(II) probably accepts an e- from the [O-O]^2- peroxide ion to give superoxide [O-O]^- which is a radical and reacts more quickly.

How do you prepare KO2 well you just heat potassium in O2 or dry air:

K + O2 → KO2

And how to we prepare metallic potassium: Na + KCl → NaCl + K ($22/kg)

http://en.wikipedia.org/wiki/Potassium

And where do we get the Na from?

"Sodium is now produced commercially through the electrolysis of liquid sodium chloride, based on a process patented in 1924. This is done in a Downs Cell in which the NaCl is mixed with calcium chloride to lower the melting point below 700 °C."

http://en.wikipedia.org/wiki/Sodium

And where do we get the energy to melt and electrolyze the NaCl?

6.022 × 10^23 windmills should do it.

I have read some references to this reaction for oxygen replenishment on space vehicles, etc.

The chemistry is fine, but what is missing from the proposal is the operating aspects:

1) where does all the KO2 come from? what is involved in producing this, particularly from a CO2 emission aspect

2) What do you do with all the K2CO3 that is produced. ?

yes it perfectly right some oxygen is also comming from the potassium oxide. I would assume there are no byproducts