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anonymous

  • 4 years ago

How many grams of magnesium oxide can be produced when 125 g Mg react with 102 g O2?

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  1. anonymous
    • 4 years ago
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    i already balenced the equation and got: 2MgO + O2 yield 2MgO

  2. JFraser
    • 4 years ago
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    Find the moles of each reactant that are available\[mol Mg = 125g Mg * (\frac{1mol Mg}{24.3g Mg})\]\[mol O{_2} = 102g O{_2} * (\frac{1mol O{_2}}{32g O{_2}})\] The reaction requires a 2:1 ratio. One of those 2 is in short supply.

  3. anonymous
    • 4 years ago
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    so is the oxygen short?

  4. anonymous
    • 4 years ago
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    ??

  5. JFraser
    • 4 years ago
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    There are 5.14 moles of Mg available, and 3.19 moles of O2 available. The ratio required is 2Mg :1O2

  6. anonymous
    • 4 years ago
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    so how do i find out the answer to the qustion?

  7. JFraser
    • 4 years ago
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    Does 5.14/3.19 = 2/1?

  8. anonymous
    • 4 years ago
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    it equals 1.611

  9. JFraser
    • 4 years ago
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    If you were going to use all 3.19 moles of O2, there would have to be twice as much Mg (6.28moles). There isn't that much available, there's only 5.14moles. The Mg will run out first. Because of that, the Mg is the limiting reactant, it will limit the amount of product you can form.

  10. anonymous
    • 4 years ago
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    i understand tht but how do i find out how much magnesium i can make

  11. JFraser
    • 4 years ago
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    Use the coefficients of the balanced reaction: 2 Mg will make 2MgO

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