A current of 2.34 A is delivered to an electrolytic cell for 85 minutes. How many grams of Au will be deposited from an aqueous solution of AuCl3?
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To find the number of grams of Au that will be deposited from an aqueous solution of AuCl3, we need to use Faraday's law of electrolysis. Faraday's law states that the amount of substance deposited or liberated at an electrode is directly proportional to the amount of electric charge passed through the cell.
The equation for Faraday's law is:
mass = (charge × molar mass) / (Faraday's constant × valence)
Where:
- mass is the mass of the substance deposited or liberated,
- charge is the electric charge passed through the cell,
- molar mass is the molar mass of the substance,
- Faraday's constant is a constant equal to 96,485 C/mol, and
- valence is the number of electrons involved in the reaction.
In this case, we are depositing Au from an aqueous solution of AuCl3. The valence of Au is 3 because each Au ion requires 3 electrons to be reduced to Au. The molar mass of Au is 196.97 g/mol.
First, we need to calculate the charge passed through the cell. To do this, we can use the equation:
charge = current × time
Given that the current is 2.34 A and the time is 85 minutes (convert to seconds by multiplying by 60), we can calculate the charge.
charge = 2.34 A × 85 minutes × 60 seconds/minute
Now that we have the charge, we can substitute it into Faraday's law equation to find the mass of Au deposited.
mass = (charge × molar mass) / (Faraday's constant × valence)
Substitute the values and calculate the mass.