A current of 4.5A is passed through a solution of gold for 1hr 45min. Calculate
To calculate the amount of gold deposited, we need to know the Faraday constant, which is 96,485 C/mol.
First, let's convert the time to seconds:
1 hour = 60 minutes * 60 seconds = 3600 seconds.
So 1 hour 45 minutes = 1 hour * 3600 seconds + 45 minutes * 60 seconds = 3600 + 2700 = 6300 seconds.
The charge passing through the solution can be calculated using the formula Q = I * t, where Q is the charge in Coulombs, I is the current in Amperes, and t is the time in seconds.
Q = 4.5 A * 6300 s = 28350 C.
Now, we can calculate the moles of gold deposited using the Faraday constant:
Moles of gold = Charge (C) / Faraday constant (C/mol).
Moles of gold = 28350 C / 96485 C/mol = 0.2935 mol.
To convert moles of gold to grams, we need to know the molar mass of gold. The molar mass of gold is 196.97 g/mol.
Mass of gold deposited = Moles of gold (mol) * Molar mass of gold (g/mol).
Mass of gold deposited = 0.2935 mol * 196.97 g/mol = 57.84 g.
Therefore, the calculated mass of gold deposited is approximately 57.84 grams.