Question

What will be the relative abundance of 63 Cu in a mixture of Cu and 6$Cu if the atomic mass of Cu in the periodic table is
63.5amu?​

Answer 1

Answer:

you know, the average atomic mass of an element is determined by taking the weighted average of the atomic masses of its naturally occurring isotopes.

Simply put, an element's naturally occurring isotopes will contribute to the average atomic mass of the element proportionally to their abundance.

avg. atomic mass

=

∑

i

(

isotope

i

×

abundance

x

)

When it comes to the actual calculation, it's easier to use decimal abundances, which are simply percent abundances divided by

100

.

So, you know that copper has two naturally occurring isotopes, copper-63 and copper-65. This means that their respective decimal abundance must add up to give

1

.

If you take

x

to be the decimal abundance of copper-63, you can say that the decimal abundance of copper-65 will be equal to

1

−

x

.

Therefore, you can say that

Explanation:

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