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4 years ago

What is the molar mass of AuCl3

Chemistry

2 answers:

azamat4 years ago

3 0

Gold(III) Chloride has an average Molar mass if 303.33g/mol.

kotykmax [81]4 years ago

3 0

Answer:

303.32557 g/mol.

Explanation:

Gold III Chloride is also known as acid gold trichloride.

PROPERTIES OF GOLD III CHLORIDE,AuCl3:

Gold III Chloride exist in colour appearance of Red crystals,and yellow crystals. It has a melting point of 254 °C and a density of

4.7 g/cm3. AuCl3 exist as a dimer( Au2Cl6) and it is somewhat covalent.

Molar mass is the the mass of one mole of a substance and is expressed in g/mol. Gold atomic mass is 196.96657, chlorine has 35.453.

Hence, molar mass of AuCl3= atomic number of Gold + atomic mass of chlorine × (number of atoms of chlorine in AuCl3).

Molar mass of AuCl3 = 196.96657 + (35.453 × 3). = 196.96657 + 106.359.

Molar mass of AuCl3= 303.32557 g/mol.

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$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

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Putting values in above equation, we get:

$9.45mol=\frac{\text{Actual yield of lithium chlorate}}{90.4g/mol}\\\\\text{Actual yield of lithium chlorate}=(9.45mol\times 90.4g/mol)=854.28g$

To calculate the theoretical yield of lithium chlorate, we use the equation:

$\%\text{ yield}=\frac{\text{Actual yield}}{\text{Theoretical yield}}\times 100$

Actual yield of lithium chlorate = 854.28 g

Percentage yield of lithium chlorate = 81.0 %

Putting values in above equation, we get:

$81=\frac{854.28g}{\text{Theoretical yield of lithium chlorate}}\times 100\\\\\text{Theoretical yield of lithium chlorate}=\frac{854.28\times 100}{81}=1054.67g$

Hence, the theoretical yield of the lithium chlorate is 1054.67 grams

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