Calculating the Number of Chlorine Atoms

Oct 13, 2025 by thesweetdesigns.com 56 views

Understanding the Chemical Formula

Gold(III) chloride, denoted as $Au_2Cl_6$ , is a chemical compound consisting of gold and chlorine atoms. The subscripts in the chemical formula indicate the number of atoms of each element present in one molecule of the compound. In this case, one molecule of gold(III) chloride contains 2 gold atoms and 6 chlorine atoms.

Determining the Molar Mass of Gold(III) Chloride

To calculate the number of chlorine atoms in a given sample of gold(III) chloride, we first need to determine the molar mass of the compound. The molar mass is the sum of the atomic masses of all the atoms present in one molecule of the compound.

The atomic mass of gold (Au) is 196.97 g/mol, and the atomic mass of chlorine (Cl) is 35.45 g/mol. Since there are 2 gold atoms and 6 chlorine atoms in one molecule of gold(III) chloride, the molar mass of the compound can be calculated as follows:

Molar mass of $Au_2Cl_6$ = (2 x atomic mass of Au) + (6 x atomic mass of Cl) = (2 x 196.97 g/mol) + (6 x 35.45 g/mol) = 393.94 g/mol + 212.7 g/mol = 606.64 g/mol

Calculating the Number of Moles of Gold(III) Chloride

Now that we have the molar mass of gold(III) chloride, we can calculate the number of moles of the compound present in a 150.0 g sample. The number of moles can be calculated using the following formula:

Number of moles = mass of sample / molar mass = 150.0 g / 606.64 g/mol = 0.247 mol

Calculating the Number of Chlorine Atoms

Since one molecule of gold(III) chloride contains 6 chlorine atoms, the total number of chlorine atoms present in the sample can be calculated by multiplying the number of moles by the number of chlorine atoms per molecule and then multiplying by Avogadro's number (6.022 x 10^23 atoms/mol).

Number of chlorine atoms = (number of moles x number of chlorine atoms per molecule) x Avogadro's number = (0.247 mol x 6) x 6.022 x 10^23 atoms/mol = 1.488 x 10^24 atoms

Rounding the Answer to 4 Significant Digits

The final answer should be rounded to 4 significant digits. Therefore, the number of chlorine atoms in a 150.0 g sample of gold(III) chloride is:

1.49 x 10^24 atoms

Conclusion

In this article, we calculated the number of chlorine atoms in a 150.0 g sample of gold(III) chloride using the chemical formula, molar mass, and Avogadro's number. The final answer was rounded to 4 significant digits, providing a precise value for the number of chlorine atoms present in the sample.

References

Atomic masses of elements: CRC Handbook of Chemistry and Physics
Avogadro's number: International Union of Pure and Applied Chemistry

Additional Resources

Chemical Formula Calculator
Molar Mass Calculator
Frequently Asked Questions (FAQs) about Calculating the Number of Chlorine Atoms in Gold(III) Chloride =============================================================================================

Q: What is the chemical formula for gold(III) chloride?

A: The chemical formula for gold(III) chloride is $Au_2Cl_6$ .

Q: What is the molar mass of gold(III) chloride?

A: The molar mass of gold(III) chloride is 606.64 g/mol.

Q: How do I calculate the number of moles of gold(III) chloride in a given sample?

A: To calculate the number of moles of gold(III) chloride, you need to divide the mass of the sample by the molar mass of the compound. For example, if you have a 150.0 g sample of gold(III) chloride, the number of moles can be calculated as follows:

Number of moles = mass of sample / molar mass = 150.0 g / 606.64 g/mol = 0.247 mol

Q: How do I calculate the number of chlorine atoms in a given sample of gold(III) chloride?

A: To calculate the number of chlorine atoms, you need to multiply the number of moles of gold(III) chloride by the number of chlorine atoms per molecule (6) and then multiply by Avogadro's number (6.022 x 10^23 atoms/mol). For example, if you have a 150.0 g sample of gold(III) chloride, the number of chlorine atoms can be calculated as follows:

Number of chlorine atoms = (number of moles x number of chlorine atoms per molecule) x Avogadro's number = (0.247 mol x 6) x 6.022 x 10^23 atoms/mol = 1.488 x 10^24 atoms

Q: Why do I need to round the answer to 4 significant digits?

A: Rounding the answer to 4 significant digits is a way to express the result with a reasonable degree of precision. In this case, the number of chlorine atoms in a 150.0 g sample of gold(III) chloride is 1.49 x 10^24 atoms.

Q: What are some common mistakes to avoid when calculating the number of chlorine atoms in gold(III) chloride?

A: Some common mistakes to avoid include:

Not using the correct chemical formula for gold(III) chloride
Not calculating the molar mass of the compound correctly
Not multiplying the number of moles by the correct number of chlorine atoms per molecule
Not rounding the answer to 4 significant digits

Q: What are some real-world applications of calculating the number of chlorine atoms in gold(III) chloride?

A: Calculating the number of chlorine atoms in gold(III) chloride has several real-world applications, including:

Determining the amount of chlorine present in a sample of gold(III) chloride
Calculating the amount of gold present in a sample of gold(III) chloride
Understanding the chemical properties of gold(III) chloride

Q: Where can I find more information about calculating the number of chlorine atoms in gold(III) chloride?

A: You can find more information about calculating the number of chlorine atoms in gold(III) chloride in various online resources, including: