An alloy is 11.1% copper by mass in tin. Copper makes up what percentage of the atoms in this sample?
To solve this problem, we need to use the atomic masses of copper and tin, which are 63.55 g/mol and 118.71 g/mol, respectively.
Let's assume we have a 100 g sample of the alloy. Then, the mass of copper in the sample would be 11.1 g (since the alloy is 11.1% copper by mass).
We can now calculate the number of moles of copper in the sample:
moles of copper = mass of copper / atomic mass of copper moles of copper = 11.1 g / 63.55 g/mol moles of copper = 0.175 moles
Similarly, we can calculate the number of moles of tin in the sample:
moles of tin = (100 g - 11.1 g) / 118.71 g/mol moles of tin = 0.743 moles
The total number of atoms in the sample is equal to the sum of the number of atoms of copper and tin:
total number of atoms = (moles of copper x Avogadro's number) + (moles of tin x Avogadro's number) total number of atoms = (0.175 mol x 6.022 x 10^23/mol) + (0.743 mol x 6.022 x 10^23/mol) total number of atoms = 4.27 x 10^23
The percentage of atoms that are copper is given by:
percentage of atoms that are copper = (number of atoms of copper / total number of atoms) x 100% percentage of atoms that are copper = (0.175 mol x 6.022 x 10^23/mol / 4.27 x 10^23) x 100% percentage of atoms that are copper = 23.1%
Therefore, copper makes up 23.1% of the atoms in this alloy.
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