what mass of gold can you extract from 34.94g of AuCl3 using electrolysis of an aqueous solution?
34.94 x (atomic mass Au/molar mass AuCl3) = ?
To find the mass of gold that can be extracted from 34.94g of AuCl3 using electrolysis, we need to calculate the molar mass of AuCl3 and then use stoichiometry to determine the mass of gold produced.
Step 1: Calculate the molar mass of AuCl3:
The molar mass of gold (Au) is 196.97 g/mol.
The molar mass of chlorine (Cl) is 35.45 g/mol (since there are 3 chlorine atoms in AuCl3).
Molar mass of AuCl3 = (molar mass of Au) + (3 * molar mass of Cl)
= (196.97 g/mol) + (3 * 35.45 g/mol)
= 196.97 g/mol + 106.35 g/mol
= 303.32 g/mol
Step 2: Determine the moles of AuCl3:
To find the moles of AuCl3, divide the given mass of AuCl3 (34.94g) by its molar mass (303.32 g/mol):
Moles of AuCl3 = (mass of AuCl3) / (molar mass of AuCl3)
= 34.94g / 303.32 g/mol
≈ 0.115 moles (rounded to three decimal places)
Step 3: Use stoichiometry to determine the moles of gold (Au):
From the balanced equation of AuCl3, we know that 1 mole of AuCl3 produces 1 mole of Au.
Moles of Au = Moles of AuCl3
≈ 0.115 moles (rounded to three decimal places)
Step 4: Convert moles of gold (Au) to mass:
Use the molar mass of gold (196.97 g/mol) to convert moles of Au to mass:
Mass of Au = Moles of Au * Molar mass of Au
= 0.115 moles * 196.97 g/mol
≈ 22.6 g (rounded to one decimal place)
Therefore, you can extract approximately 22.6 grams of gold from 34.94 grams of AuCl3 using electrolysis of an aqueous solution.