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anonymous

  • one year ago

Find the mass in grams of 2.00*10^23 molecules of F2.

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  1. anonymous
    • one year ago
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    \[2.00 \times 10^{23} molecules F _{2} \times \frac{ 1mol F _{2} }{ 6.023 \times 10^{23} molecules F _{2} } \times \frac{ 38.00 g F _{2} }{ 1mol F _{2} }\]

  2. anonymous
    • one year ago
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    1molF2, would that be the atomic mass or Fluorine times 2?

  3. anonymous
    • one year ago
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    Yep. 1 mole is atomic mass.

  4. anonymous
    • one year ago
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    would the answer be 1.26*10^47?

  5. anonymous
    • one year ago
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    If you calculated it right, it would be.

  6. anonymous
    • one year ago
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    Okay, thank you very much!!

  7. anonymous
    • one year ago
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    Doenst look like it to me. It should be less.

  8. anonymous
    • one year ago
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    It should be way way less. The grams should be less than 38 grams.

  9. anonymous
    • one year ago
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    on my calculator I typed in 2.00*10^23 x 37.996/6.022*10^23 x 38.00/37.996 = 1.26203919*10^47

  10. anonymous
    • one year ago
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    Where are you getting those numbers? Use my dimensional analysis. As you can see the given unit is canceled out and the mass unit (grams) is left. No need to add anything.

  11. anonymous
    • one year ago
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    I did use it. I replace 1molF2 w/ 37.996, thats the only thing that is different!

  12. anonymous
    • one year ago
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    I got that by doing: (2*18.998) = 37.996

  13. anonymous
    • one year ago
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    Close enough to be 38.00 gram. Thats why I put it on top of mole. 1 mole F2=38.00 grams F2 You dont replace anything in this conversion. You can but its not necessary. Just makes everything longer. And you are not entering it in the calculator right because of the unnecessary steps. (2.00 x 10^23/6.023 x 10^23) x 38.00 This is just basic operations.

  14. anonymous
    • one year ago
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    okay well thank you

  15. anonymous
    • one year ago
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    No problem!

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