Question

Calculate the number of gold atoms in a 80.0 g sample of gold(III) chloride \( \left(\mathrm{Au}_{2} \mathrm{Cl}_{6}\right) \). Be sure your answer has a unit symbol if necessary, and round it to 3 significant digits. \( \square \) \( \square \) 40

          Calculate the number of gold atoms in a 80.0 g sample of gold(III) chloride \( \left(\mathrm{Au}_{2} \mathrm{Cl}_{6}\right) \).
Be sure your answer has a unit symbol if necessary, and round it to 3 significant digits.
\( \square \)
\( \square \) 40

Calculate the number of gold atoms in a 80.0 g sample of gold(III) chloride (Au2Cl6).
Be sure your answer has a unit symbol if necessary, and round it to 3 significant digits.
□
□ 40

Added by Margaret P.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Jeremy Higgins

Step 1

- Gold (Au) has an atomic mass of approximately 197.0 g/mol. - Chlorine (Cl) has an atomic mass of approximately 35.5 g/mol. Calculate the molar mass: \[ \text{Molar mass of } \mathrm{Au}_{2}\mathrm{Cl}_{6} = 2(197.0) + 6(35.5) = 394.0 + 213.0 = 607.0 \, Show more…

Show all steps

Thanks for your feedback!

Calculate the number of gold atoms in a 80.0 g sample of gold(III) chloride \( \left(\mathrm{Au}_{2} \mathrm{Cl}_{6}\right) \). Be sure your answer has a unit symbol if necessary, and round it to 3 significant digits. \( \square \) \( \square \) 40