Topic: Isotopic Fractionation
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How to Find Fractional Abundance of an Isotope
Isotopes of a particular element are atoms that contain the same number of protons and electrons but have a different number of neutrons. Due to the added neutrons, these atoms have a different atomic mass. This variation in mass, however, ... Read More »
Source: http://www.ehow.com/how_8646998_fractional-abundance-isotope.html
What is isotope fractionation?
( ′ī·sə′tōp ′frak·shə¦nā·shən ) (nucleonics) Natural or artificial alteration of the isotopic composition of an element via processes of diffusion, evaporation, and chemical exchange, utilizing small differences in physical and chemical pro... Read More »
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What part of speech is isotope fractionation?
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Isotopic Fractionation
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I think you mean the isotope fraction of lead, that is why the question has been edited. Lead has 4 isotopes that are considered stable: Pb 204, Pb 206 , Pb 207 and Pb 208. Out of these four Pb 204 is not the result of any radioactive decay...
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Source: http://www.enotes.com/science/q-and-a/what-isotope-function-lead-...
Multiply number of x adn ave mass per x
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Source: http://wiki.answers.com/Q/How_ca_you_find_the_fractional_abundanc...
It depends on the half life of the isotope. If the half life is, for example, 10 minutes, then 1/8 of the parent isotope will remain (30/10 = 3; 1/2^3 = 1/8). Essentially, to work out the remaining fraction, you firstly divide the period of...
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Source: http://wiki.answers.com/Q/What_fraction_of_the_parent_isotope_wil...
For each isotope, divide the individual mass by the ...
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Source: http://www.chacha.com/question/what-is-the-fractional-abundance-o...
we say that if Re-185 is X% the fractional abundance of Re-187 is (100 -X) then X% of 184.95 amu & (100 -X)% of 186.96 = 186.21 amu 184.95 X & 186.96 - 186.96X = 186.21 - 2.01X = - 0.75 X = 0.3731 .... aka 37.31 % Re-185 your answers are 37...
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Source: http://answers.yahoo.com/question/index?qid=20100127124039AAp0ivM
I'm assuming that you already know the masses of the isotopes in a sample. Call them M1, M2, M3 etc. 1. Add them all up to get the grand total of the number of grams of all of the isotopes put together. Call this intermediate result Mt. 2. ...
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Source: http://answers.yahoo.com/question/index?qid=20081020102440AAU511w
