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andre [41]
3 years ago
12

Sodium only has one naturally occuring isotope, Na23 , with a relative atomic mass of 22.9898 u. A synthetic, radioactive isotop

e of sodium, Na22 , is used in positron emission tomography. Na22 has a relative atomic mass of 21.9944 u.
A 1.5909 g sample of sodium containing a mixture of Na23 and Na22 has an apparent "atomic mass" of 22.9785 u . Find the mass of Na22 contained in this sample
Chemistry
1 answer:
NISA [10]3 years ago
4 0

Answer:

0.000399316  g

Explanation:

We can start with the <u>molar fraction</u> for each isotope:

We can say that the abudandance of ^2^3Na is an unknow value <u>"X"</u> and the molar fraction of ^2^2Na is <u>"Y"</u>. We have to keep in mind that the molar fractions can be added:

Y + X = 1

So, we can put the molar fraction of ^2^2Na in terms of ^2^3Na, so:

Y=1-X

So, we will have the <u>molar fraction of each isotope</u>:

^2^2Na: X-1

^2^3Na: X

And the <u>atomic mass</u>:

^2^2Na: 21.9944

^2^3Na: 22.9898

If we multiply the molar mass by the each atomic mass of each isotope we will have:

22.9898*(X)~+~21.9944*(X-1)~=~22.9785

Now we can solve for "X" :

22.9898X~+~21.9944X~-21.9944~=~22.9785

44.9842X-21.9944~=~22.9785

44.9842X~=~22.9785~+~21.9944&#10;

44.9842X~=~44.9729&#10;

X~=~\frac{44.9729}{44.9842}

X~=~0.999749&#10;

The molar fraction of ^2^3Na is <u>0.999749</u>. Now we can calculate the molar fraction of ^2^2Na, so:

Y~=~1-0.999749~=~0.000251&#10;

Now, if we multiply the molar fraction by the mass we can find the <u>mass</u> of ^2^2Na, so:

mass~of~^2^2Na~=~1.5909~g*0.000251~=~0.000399316~&#10;g

The mass of ^2^2Na is 0.000399316  g

I hope it helps!

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