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Need help on Isotopes

  1. Apr 2, 2010 #1
    1. The problem statement, all variables and given/known data
    I have been working on this for ages and can't work it out.
    Naturally occurring antimony (Sb) has a molar mass of 121.84 g/mol and contains only two isotopes. One is 121Sb which is 57.3% abundant. What is the mass number of the other isotope of naturally occurring antimony?

    I have been through all my text books and can't find the answer, have also googled and I am totally stuck. I need to show how I came to my answer. I don't need to have the question done for me just how to go about working it out.
    Thanks in advance for any help.



    2. Relevant equations



    3. The attempt at a solution
     
  2. jcsd
  3. Apr 3, 2010 #2

    phyzguy

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    Science Advisor

    The molar mass is the average mass of all of the isotopes. If 57% is 121, what must the other one isotope be in order for the average to be 121.84?
     
  4. Apr 5, 2010 #3

    epenguin

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    Gold Member

    Yes, it's got to be a small whole number, now just over 40% if this other isotope adds 0.84 to the average, I think I can work out what it must be in my head, and if not just try 1, 2, 3,... you will never have to go very far.
     
  5. Apr 6, 2010 #4
    I don't follow your reasoning; the number must be greater than 121 for the average to be 0.84 higher with a lower abundance. I may just be misunderstanding, so sorry=]

    allie, I'll assume you know how to take the average mass of two isotopes, but you may not have looked at the full equation for the mass; maybe this'll help :)

    in this case [tex]\frac{(121 \times 57.3) + (M \times (100-57.3))}{100} = 121.84[/tex]
     
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