What quantity in moles of silver atoms do you have if you have 5.08 × 1021 atoms of silver. (The mass of one mole of silver is 107.87 g.)

Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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**Question:**

What quantity in moles of silver atoms do you have if you have \(5.08 \times 10^{21}\) atoms of silver? (The mass of one mole of silver is 107.87 g.)

**Explanation:**

To find the number of moles, use Avogadro's number, which is \(6.022 \times 10^{23}\) atoms/mole. The formula to calculate moles is:

\[
\text{Moles of silver} = \frac{\text{Number of atoms}}{\text{Avogadro's number}}
\]

Substitute the given number of atoms:

\[
\text{Moles of silver} = \frac{5.08 \times 10^{21}}{6.022 \times 10^{23}}
\]

Finally, solve for the quantity in moles. This formula provides a conversion from atoms to moles using a fundamental constant in chemistry.
Transcribed Image Text:**Question:** What quantity in moles of silver atoms do you have if you have \(5.08 \times 10^{21}\) atoms of silver? (The mass of one mole of silver is 107.87 g.) **Explanation:** To find the number of moles, use Avogadro's number, which is \(6.022 \times 10^{23}\) atoms/mole. The formula to calculate moles is: \[ \text{Moles of silver} = \frac{\text{Number of atoms}}{\text{Avogadro's number}} \] Substitute the given number of atoms: \[ \text{Moles of silver} = \frac{5.08 \times 10^{21}}{6.022 \times 10^{23}} \] Finally, solve for the quantity in moles. This formula provides a conversion from atoms to moles using a fundamental constant in chemistry.
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