Answer:
0.043 grams of mercury metal will be deposited from the solution containing Hg²⁺ ions if a current of 1.25 A is applied for 54.6 minutes.
Step-by-step explanation:
To calculate the grams of mercury metal deposited, we need to use Faraday's law of electrolysis. According to Faraday's law, the amount of substance deposited at an electrode is directly proportional to the quantity of electricity passed through the cell.
The formula to calculate the amount of substance deposited is:
Amount of substance (in moles) = (current (in amperes) × time (in seconds))/F
Where F is the Faraday constant, which is approximately 96,485 coulombs per mole.
First, let's convert the time given in minutes to seconds:
Time = 54.6 minutes × 60 seconds/minute = 3276 seconds
Next, we can calculate the amount of substance deposited in moles:
Amount of substance (in moles) = (1.25 A × 3276 s)/96485 C/mol
Now, we need to determine the molar mass of mercury (Hg). The molar mass of mercury is approximately 200.59 g/mol.
Finally, we can calculate the grams of mercury deposited using the molar mass:
Grams of mercury deposited = Amount of substance (in moles) × Molar mass (in grams/mole)
Grams of mercury deposited = (1.25 A × 3276 s)/96485 C/mol × 200.59 g/mol
Performing the calculation:
Grams of mercury deposited = 0.043 g
Therefore, approximately 0.043 grams of mercury metal will be deposited from the solution containing Hg²⁺ ions if a current of 1.25 A is applied for 54.6 minutes.