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What mass of water, in grams, would have to be decomposed to produce 13.3 L of molecular oxygen at STP?

How do I go about doing this problem?

  • Chemistry -

    how many moles is that?

    n=PV/RT solve that.

    Then, each mole of water decomposes to 1/2 mole of oxygen gas. so whatever moles of O2 you found, multipy by two, that is the moles of water, convert that to grams.

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