Posted by **Laila** on Monday, February 23, 2009 at 8:55pm.

The element copper, found in nature with an average atomic mass of 63.54u, consists of two isotopes, copper-63 of atomic mass 62.93u and copper-65 of atomic mass 64.93u. Calculate the abundance of each isotope.

I can't come up with an equation to solve it; can someone please help with this?

- Chemistry -
**DrBob222**, Monday, February 23, 2009 at 9:21pm
62.93*(x) + 64.93*(1-x) = 63.54

where x is decimal equivalent for that isotope and 1-x for the other isotope.

- Chemistry -
**GK**, Monday, February 23, 2009 at 9:31pm
Let the fraction of Copper-65 = x.

Then Copper-63 would be (1-x)

We set up an equation for the "weighted average" of copper based on the individual isotopes of copper:

62.93(1-x) + 64.93x = 63.54

Solve for x to get the % of Cu-63

Use (1-x) to get the % of Cu-65

- Chemistry -
**Laila**, Monday, February 23, 2009 at 9:59pm
oh ok, I solved it, thank you very much! :]

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