When 0.340 mol of butane, C4H10, are burned with excess oxygen giving CO2 and H2O, how many moles of oxygen are consumed?

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  1. balance the equation. I bet you get four moles of CO2 and 5 moles of water for each mole of butane. If that is true, then you must use 4O2+5(1/2O2) of oxygen, or 6.5 moles O2 for each mole of butane. So you had .340moles, and that multiplied by 6.5 is ...

    Balance the equation and see

  2. wrong

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  3. 12

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  4. 13.0

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