Calcalate the mass of silver deposited when a current of 2.6A is passed through a solution silver salt for 70mins?
coulombs = amperes x seconds
coulombs = 2.6 A x 70 min x (60 sec/min) = approx 11,000 C but you should use a better number than that.
96,485 coulombs will deposit 107.9 grams of Ag. Therefore, 11,000 C will deposit
107.9 g Ag x (11,000/96,485) = ? g Ag deposited.
Remember to start from scratch and recalculate each step above.
Well, if you want me to take this question seriously, I'd say that to calculate the mass of silver deposited, we need to consider the relationship between current, time, and the amount of substance deposited. This relationship is given by Faraday's law of electrolysis.
According to Faraday's law, the quantity of silver deposited is directly proportional to the current and the time. The proportionality constant is the electrochemical equivalent of silver, which is 0.001118 kg/C.
So, to calculate the mass of silver deposited, we can use the formula:
Mass of silver = electrochemical equivalent × current × time
Substituting the given values, we have:
Mass of silver = 0.001118 kg/C × 2.6 A × 70 mins
Now you just have to plug in the values and do the math!
But let's be real, if you pass a current of 2.6A through a silver salt solution, you'll probably end up with a very shocked solution! Better be careful with your experiments!
To calculate the mass of silver deposited, we can use Faraday's law of electrolysis, which states that the amount of substance (in this case, silver) deposited or produced during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte.
The equation can be written as:
Mass (in grams) = (Current (in Amperes) × Time (in seconds) × Atomic Mass of Silver) / (Faraday's Constant)
First, let's convert the time from minutes to seconds:
70 minutes = 70 * 60 = 4200 seconds
Next, we need to determine the atomic mass of silver. The atomic mass of silver (Ag) is approximately 107.87 g/mol.
Lastly, we need to know Faraday's constant, which is the charge on one mole of electrons. Faraday's constant is approximately 96,485 Coulombs per mole of electrons.
Now, we can calculate the mass of silver deposited:
Mass (in grams) = (2.6 A × 4200 s × 107.87 g/mol) / (96,485 C/mol)
Let's plug in the values and calculate:
Mass (in grams) = (2.6 A × 4200 s × 107.87 g/mol) / 96,485 C/mol
Mass (in grams) = 0.938 g
Therefore, the mass of silver deposited when a current of 2.6 A is passed through a silver salt solution for 70 minutes is approximately 0.938 grams.
To calculate the mass of silver deposited, you need to use Faraday's law of electrolysis. Faraday's law states that the amount of substance deposited or liberated during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte.
Here is the step-by-step process to calculate the mass of silver deposited:
1. Determine the flow of current (I) in amperes (A): In this case, the current is given as 2.6 A.
2. Calculate the total charge passed (Q): To get the total charge, you need to convert the time from minutes to seconds. As there are 60 seconds in a minute, 70 minutes would be equivalent to 70 x 60 = 4200 seconds. Therefore, the total charge (Q) can be calculated using the formula:
Q = I * t
= 2.6 A * 4200 s
= 10,920 Coulombs (C)
3. Convert the charge to moles of electrons: The charge passed is equal to the number of moles of electrons (n) multiplied by the Faraday constant (F), which is approximately 96,485 C/mol. Rearranging the equation, you can solve for n:
n = Q / F
= 10,920 C / 96,485 C/mol
≈ 0.113 mol
4. Determine the molar ratio based on the balanced chemical equation: For each mole of silver deposited, one mole of electrons is consumed. The balanced chemical equation for the deposition of silver is:
Ag⁺(aq) + e⁻ → Ag(s)
Therefore, the molar ratio of Ag⁺ to e⁻ is 1:1.
5. Calculate the molar mass of silver: The molar mass of silver (Ag) is approximately 107.87 grams/mole.
6. Determine the mass of silver deposited (m): Multiply the number of moles (n) by the molar mass of silver (M):
m = n * M
= 0.113 mol * 107.87 g/mol
≈ 12.20 grams
So, approximately 12.20 grams of silver would be deposited when a current of 2.6A is passed through the silver salt solution for 70 minutes.