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Calculate the number of gold atoms in a 80.0 g sample of gold (III) chloride (Au2CI6)Be sure your answer has a unit symbol if necessary, and rounded to 3 significant digits

Calculate The Number Of Gold Atoms In A 800 G Sample Of Gold III Chloride Au2CI6Be Sure Your Answer Has A Unit Symbol If Necessary And Rounded To 3 Significant class=

Sagot :

The number of gold atoms is 1.590x10^23.

- First, with the molar mass of Au2Cl6 (607g/mol) we can find the grams of Au in 80g of Au2Cl6:

[tex]\begin{gathered} 607g\text{ of Au2Cl6 \_\_\_\_\_\_ 394g of Au} \\ 80g\text{ of Au2Cl6 \_\_\_\_\_\_ x= }\frac{80g.394g}{607g} \\ x=\text{ 51.93g} \end{gathered}[/tex]

Now we know that there are 51.93g of Au in 80g of Au2Cl6.

- Second, with the molar mass of gold (197g/mol) we can calculate the number of moles in 51.93g of gold:

[tex]\begin{gathered} 197g\text{ \_\_\_\_\_ 1mol} \\ 51.93g\text{ \_\_\_\_ x= }\frac{51.93g.1mol}{197g} \\ x=0.264\text{mol} \end{gathered}[/tex]

Now we know that there are 0.264 moles of gold in the sample.

- Third, with the Avogadro's number (6.022*10^23) we can calculate the number of gold atoms in the sample:

[tex]\frac{0.264mol.\mleft(6.022x10^{23}\mright)}{1\text{mol}}=1.590x10^{23}[/tex]

So, the number of gold atoms is 1.590x10^23.

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