Calculate the mass of silver deposited when a current of 2.6 A ls passed through a solution of silver salt for 70 minutes. (Ag=108; 1 faraday=96 500 c)
m1=108g
shaibu
12.22
Calculate the mass of silver deposited when a current
To calculate the mass of silver deposited, we can use Faraday's law of electrolysis, which states that the amount of substance deposited or released at an electrode is directly proportional to the quantity of electric charge passed through the electrolyte.
The formula we will use is:
Mass = (Electrochemical equivalent) x (Current) x (Time)
Let's break down the information given:
Current (I) = 2.6 A
Time (t) = 70 minutes
First, we need to convert the time from minutes to seconds, as current is given in amperes per second.
Time (t) = 70 minutes x (60 seconds/1 minute)
= 4200 seconds
Now, we need to find the electrochemical equivalent (chemical equivalent) of silver. The electrochemical equivalent represents the amount of substance deposited for a given amount of charge.
Given:
Ag = 108 g/mol (molar mass of silver)
1 faraday (F) = 96,500 C (charge in coulombs)
To find the electrochemical equivalent, we need to determine the number of moles of silver for 1 faraday of charge.
1 mol of silver (Ag) corresponds to 1 faraday of charge.
108 g of silver (Ag) corresponds to 1 mol of silver.
Thus, the molar mass of silver (Ag) corresponds to the amount of charge in 1 faraday:
Molar mass of silver (Ag) = 108 g/mol
Charge in 1 faraday (F) = 96,500 C
Now, let's calculate the electrochemical equivalent of silver:
Electrochemical equivalent (E) = Molar mass / Charge in 1 faraday
= 108 g/mol / 96,500 C
Next, we can substitute the values into the formula:
Mass = Electrochemical equivalent x Current x Time
Mass = (108 g/mol / 96,500 C) x (2.6 A) x (4200 seconds)
Calculating this, we get:
Mass ≈ 0.003011 g
Therefore, the mass of silver deposited when a current of 2.6 A is passed through a solution of silver salt for 70 minutes is approximately 0.003011 grams.