The element copper exists in nature as two isotopes: has a mass of 62.9296 u and has a mass of 64.9278 u. The average atomic mass of copper is 63.55 u. Calculate the relative abundance of the two copper isotopes.

%isotope 1 = 68.92%

%isotope 2 = 31.08 %

Explanation:

we have the following data:

misotope 1 = 62.9296 u

misotope 2 = 64.9278 u

maverage = 63.55 u

%isotope 1 = X

%isotope 2 = 100-X

the average atomic mass is equal to:

maverage = [(misotope 1x%isotope 1)+(misotope 2x%isotope 2)/100]

substituting values:

63.55 = [(62.9296 x X)+(64.9272 x (100-X))]/100

clearing the X:

X = 68.92

therefore we have to:

%isotope 1 = 68.92%

%isotope 2 = 100-68.92 = 31.08 %

elements make up everything, and they combine to make compounds.

the answer is c