an aqueous solution of pdcl2 is electrolyzed for 27.4 seconds during this time 0.1064 g of Pd is deposited on the cathode. Calculate the average current used in the electrolysis.
The average current used in the electrolysis can be calculated using the following equation:
Average current = (mass of Pd deposited/time) / (charge of Pd ion)
Average current = (0.1064 g/27.4 s) / (2 x 1.602 x 10^-19 C)
Average current = 0.945 A
To calculate the average current used in the electrolysis, we can use Faraday's law of electrolysis, which states that the amount of substance deposited or liberated at an electrode is directly proportional to the quantity of electricity passed through the cell.
The equation to calculate the average current (I) is:
I = Q / t
Where:
I = average current (in Amperes)
Q = quantity of electricity (in Coulombs)
t = time (in seconds)
To find the quantity of electricity (Q), we need to determine the number of moles of Pd deposited using the molar mass of Pd, and then convert it to Coulombs using Faraday's constant.
1. Calculate the number of moles of Pd deposited:
Given: Mass of Pd (m) = 0.1064 g
Molar mass of Pd (M) = 106.42 g/mol
Number of moles (n) = m / M
n = 0.1064 g / 106.42 g/mol
n ≈ 0.001000 mol
2. Convert moles to Coulombs:
Using Faraday's constant (F) = 96485 C/mol (1 mole of electrons = 96485 Coulombs)
Quantity of electricity (Q) = n * F
Q = 0.001000 mol * 96485 C/mol
Q ≈ 96.485 C
3. Calculate the average current (I):
Given: Time (t) = 27.4 seconds
I = Q / t
I = 96.485 C / 27.4 s
I ≈ 3.525 Amperes
Therefore, the average current used in the electrolysis is approximately 3.525 Amperes.
To calculate the average current used in the electrolysis, we need to use Faraday's law of electrolysis, which states that the amount of substance deposited or liberated at an electrode is directly proportional to the quantity of electricity passed through the electrolyte.
The formula to calculate the average current (I) is:
I = Q / t
where I is the average current, Q is the total charge passed, and t is the time in seconds.
First, we need to calculate the total charge passed (Q). We can use the formula:
Q = n * F
where Q is the total charge passed, n is the number of moles of electrons transferred, and F is Faraday's constant.
To determine the number of moles of electrons transferred (n), we can use the balanced chemical equation for the electrolysis of PdCl2:
PdCl2(aq) -> Pd(s) + Cl2(g)
From the equation, we can see that for every mole of Pd deposited, 2 moles of electrons are transferred. So, if we know the amount of Pd deposited, we can calculate the number of moles of electrons.
The molar mass of Pd is 106.42 g/mol. Therefore, the number of moles of Pd deposited can be calculated using the equation:
moles of Pd = mass of Pd / molar mass of Pd
moles of Pd = 0.1064 g / 106.42 g/mol
Next, we can calculate the total charge passed using the equation:
Q = n * F
Q = (moles of Pd * 2) * F
Faraday's constant, F, is equal to 96,485 C/mol.
Finally, we can calculate the average current using the equation:
I = Q / t
Substituting the values into the equation will give us the average current used in the electrolysis.