Posted by **Bradley** on Wednesday, July 13, 2011 at 10:15pm.

Question: What mass of water, in grams, would have to be decomposed to produce 17.6 L of molecular oxygen at STP?

Work:

n=PV/RT

x=(1 atm)(17.6 L)/(0.0821)(273 k)

x = 1.27348295454546

1.27348295454546 x 2 = 2.54696590909092

Grams= Moles x 18.0

Grams = 2.54696590909092 x 18.0

Grams = 45.8

I think I'm messing up somewhere, but I don't know what I'm doing wrong.

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