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anonymous

  • one year ago

Use the information for the isotopes of X to calculate the average atomic mass of X, and identify the element. Isotope Abundance Mass (amu) 6X 7.5% 6.015 7X 92.5% 7.016 I'm kinda confused :/

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  1. Zale101
    • one year ago
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    \(Average ~atomic~ mass~ of~ an ~element\) = \( (Abundance~percentage_1*Mass~of~Isotope~ 1)\) + \((Abundance~percentage_2*Mass~of~Isotope~ 2))\)

  2. anonymous
    • one year ago
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    So would I have to calculate that like 7.5 * 6.015, and the same for the other one?

  3. Photon336
    • one year ago
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    You would add the two masses together

  4. Zale101
    • one year ago
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    Correct. You'll add it with Isotope 7x to get the average atomic mass of the element

  5. Photon336
    • one year ago
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    but first you need to multiply the atomic mass by the % abundance I believe

  6. anonymous
    • one year ago
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    So it's 45.1125 + 648.98 ?

  7. anonymous
    • one year ago
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    @Photon336 would it be 694.0925?

  8. Photon336
    • one year ago
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    @Zale101 6X and 7X are just the names of the isotopes right?

  9. Zale101
    • one year ago
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    I believe so.

  10. anonymous
    • one year ago
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    Yeah they are...

  11. Photon336
    • one year ago
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    yeah.. so convert 7.5% to decimal form which is 7.5/100 then you multiply this by 6.015 amu

  12. Photon336
    • one year ago
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    remember @flatouthero its' a percentage

  13. anonymous
    • one year ago
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    Oh, so it's 6.94

  14. Zale101
    • one year ago
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    Correct!

  15. Zale101
    • one year ago
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    :)

  16. Zale101
    • one year ago
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    What element is that?

  17. anonymous
    • one year ago
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    Thank you both for your help!

  18. Photon336
    • one year ago
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    no problem

  19. anonymous
    • one year ago
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    Lithium, btw xD

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