Question
Copper has two naturally occurring isotopes, $^{63} \mathrm{Cu}$ (isotopicmass $=62.9296$ amu) and of Cu (isotopic mass $=64.9278$ amu). If copper has an atomic mass of 63.546 amu, what is the percent abundance of each isotope?
Step 1
Step 1: Let's denote the percent abundance of $^{63} \mathrm{Cu}$ as $x$ and the percent abundance of $^{65} \mathrm{Cu}$ as $1-x$ (since the total abundance must be 100%). Show more…
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Copper has two naturally occurring isotopes, ${ }^{6} \mathrm{Cu}$ (isotopic mass $=62.9296 \mathrm{amu}$ ) and ${ }^{65} \mathrm{Cu}$ (isotopic mass $=64.9278$ amu . If copper has an atomic mass of 63.546 amu, what is the percent abundance of each isotope?
There are 2 isotopes of copper that occur naturally; 63Cu and 65Cu. The 63Cu atoms have a mass of 62.929601 amu and the 65Cu atoms have a mass of 64.927794 amu. What is the percent natural abundance for each isotope?
Only two isotopes of copper occur naturally, ${ }^{63} \mathrm{Cu}$ (atomic mass $=62.9296$ amu; abundance $69.17 \%)$ and ${ }^{65} \mathrm{Cu}$ (atomic mass $=64.9278$ amu; abundance $30.83 \%) .$ Calculate the atomic weight (average atomic mass) of copper.
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