Problem: Only two isotopes of copper occur naturally, 63 Cu (atomic mass = 62.9296  amu; abundance 69.17 %) and 65 Cu (atomic mass = 64.9278  amu; abundance 30.83 %).Calculate the atomic weight (average atomic mass) of copper.

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FREE Expert Solution

We are asked to determine the atomic weight (average molecular mass) of a Copper (Cu) given 63 Cu (atomic mass = 62.9296  amu; abundance 69.17 %) and 65 Cu (atomic mass = 64.9278  amu; abundance 30.83 %).


We will solve for atom’s average mass using their abundance. 

The formula for average mass is:

Average molecular mass = (Mass isotope × Fractional Abundance)

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Problem Details

Only two isotopes of copper occur naturally, 63 Cu (atomic mass = 62.9296  amu; abundance 69.17 %) and 65 Cu (atomic mass = 64.9278  amu; abundance 30.83 %).

Calculate the atomic weight (average atomic mass) of copper.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Isotopes concept. You can view video lessons to learn Isotopes. Or if you need more Isotopes practice, you can also practice Isotopes practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Rabinovich's class at UNC.