Calculate the mass of silver deposited when a current of 2.2A is passed through a solution of silver salt for 80 minutes.(Ag=108,1 farasay=96500c)
Coulombs = amperes x seconds
C = 2.2 A x 80 minutes x (60 sec/min) = 10,560
You know that 108 g Ag will be deposited with 96,500 Coulombs and you have 10,560 so
108 g Ag x (10, 560/96,500) = ? g Ag
Please help me solve it
To calculate the mass of silver deposited, we need to use Faraday's Law of Electrolysis, which states that the mass (m) of a substance deposited or liberated during electrolysis is directly proportional to the electric charge (Q) and the molar mass (M) of that substance.
The formula for calculating the mass of a substance deposited during electrolysis is:
m = (Q * M) / (n * F)
Where:
m = mass of the substance deposited (in grams)
Q = electric charge passed through the solution (in Coulombs)
M = molar mass of the substance (in grams/mol)
n = number of moles of electrons involved in the reaction
F = Faraday's constant (96500 C/mol)
In this case, we are depositing silver (Ag), so the molar mass of silver (M) is 108.1 g/mol. Since silver has a +1 charge (Ag+), the number of moles of electrons involved (n) is also 1.
Given:
Electric current (I) = 2.2 A
Time (t) = 80 minutes = 80 * 60 seconds
Faraday's constant (F) = 96500 C/mol
First, let's calculate the electric charge (Q) passed through the solution:
Q = I * t
Q = 2.2 A * (80 * 60 s)
Q = 2.2 A * 4800 s
Q = 10560 C
Now, we can substitute the values into the formula to find the mass of silver deposited:
m = (Q * M) / (n * F)
m = (10560 C * 108.1 g/mol) / (1 * 96500 C/mol)
m = 1142688 gC / 96500 C/mol
m = 11.85 g
Therefore, the mass of silver deposited when a current of 2.2 A is passed through the solution for 80 minutes is approximately 11.85 grams.
To calculate the mass of silver deposited, we can use Faraday's Laws of Electrolysis.
Faraday's First Law states that the mass of any substance deposited or liberated at an electrode during electrolysis is directly proportional to the number of moles of electrons transferred during the process.
The formula to calculate the mass of a substance deposited is given by:
Mass = (Current * Time) / (Faraday's Constant * Charge of the Ion)
Where:
- Mass is the mass of the substance deposited in grams.
- Current is the current passed through the solution in amperes.
- Time is the time for which the current is passed through the solution in seconds.
- Faraday's Constant is the value 96500 coulombs per mole of electrons.
- Charge of the Ion represents the number of moles of electrons involved in the reaction.
In this case, we want to calculate the mass of silver deposited. The charge of silver ion (Ag+) is equivalent to the charge of one electron since it loses one electron to form a stable ion.
Thus, the charge of the silver ion is 1.
Now, let's calculate the mass of silver deposited:
Mass = (Current * Time) / (Faraday's Constant * Charge of the Ion)
= (2.2 A * (80 minutes * 60 seconds/minute)) / (96500 C/mol * 1 e-)
= (2.2 * 4800) / (96500)
= 0.109 g
Therefore, the mass of silver deposited when a current of 2.2A is passed through the solution of silver salt for 80 minutes is 0.109 grams.