How many seconds does it take to deposit 81.5 g of Zn on a steel gate when 21.0 A is passed through a ZnSO4 solution?
It takes 96,485 coulombs to deposit 65.4g/2 = estimated 33 g Zn
You want 81.5 g so that will require how many coulombs?
That's 96,485 x (81.5/33) = ? C.
Then C = amperes x seconds.
You know C and amperes, solve for seconds. Remember that 33 g is an estimate so you need to use more accurate values.
kjbfdksajhf
Well, you know what they say, time flies when you're depositing zinc on a steel gate! Let's calculate it. To determine the time it takes to deposit the zinc, we need to use Faraday's law of electrolysis. According to the law, the amount of substance deposited is directly proportional to the charge passed through the solution.
First, we need to calculate the charge passed through the solution using the formula:
Charge (C) = Current (A) x Time (s)
Since we're given the current (21.0 A), we can rearrange the formula to solve for time:
Time (s) = Charge (C) / Current (A)
Next, we need to find the total charge needed to deposit 81.5 g of zinc. To do that, we'll use the formula:
Charge (C) = moles x Faraday constant
Knowing that the molar mass of zinc (Zn) is approximately 65.4 g/mol and the Faraday constant is approximately 96,485 C/mol, we can solve for the moles:
moles = mass (g) / molar mass (g/mol)
Finally, we can combine the equations above to find the time it takes to deposit the zinc:
Time (s) = (mass (g) / molar mass (g/mol)) x Faraday constant (C/mol) / current (A)
Plugging in the given values:
Time (s) = (81.5 g / 65.4 g/mol) x 96,485 C/mol / 21.0 A
After crunching the numbers, the result is approximately 197,508 seconds. So, it would take approximately 197,508 seconds to deposit 81.5 g of Zn on the steel gate with a current of 21.0 A. Just enough time for a nice cup of coffee and a funny joke!
To determine the time it takes to deposit 81.5 g of Zn on a steel gate, we need to use Faraday's laws of electrolysis. The formula to calculate the mass of the substance deposited during electrolysis is:
Mass = (Current × Time × Molar Mass) / (Faraday's Constant × Valence)
Firstly, we need to find the number of moles of Zn using the given mass and molar mass. The molar mass of Zn is 65.38 g/mol.
Number of Moles = Mass / Molar Mass
Number of Moles = 81.5 g / 65.38 g/mol
Number of Moles ≈ 1.245 mol
Next, we need to determine the valence of Zn. Zinc (Zn) has a valence of 2.
Using Faraday's constant, which is equal to 96,485 C/mol, we can find the total charge passed through the circuit.
Charge = Current × Time
Solving for time:
Time = Charge / Current
Now, we can substitute these values into the equation to find the time.
Time = (Number of Moles × Faraday's Constant × Valence) / (Current × Molar Mass)
Plugging in the values:
Time = (1.245 mol × 96,485 C/mol × 2) / (21.0 A × 65.38 g/mol)
Calculating this expression will give us the time required to deposit 81.5 g of zinc on the steel gate when 21.0 A is passed through a ZnSO4 solution.