Calculate the current that must be passed into a solution of aluminum salt for 1 hours 30 minutes, in order to deposit 1.5g of aluminum where aluminum is 27
I don't have an answer but I need the answer to the question calculate the current that must be deposited or passed into a solution of aluminium salt for 1hour 30minutes in order to deposit 1.5g of aluminium (Al=27)
To calculate the current required to deposit 1.5g of aluminum, we need to use the Faraday's law of electrolysis, which states that the amount of substance deposited is directly proportional to the charge passed through the solution.
The molar mass of aluminum is 27 g/mol, so 1.5g of aluminum is approximately (1.5/27) = 0.056 mol.
The Faraday's constant is 96,485 C/mol.
Now, we can use the equation:
Coulombs = current (A) x time (s)
We have the time given as 1 hour 30 minutes, which is equivalent to (1 hour + 30 minutes) = (1 x 60 x 60) + (30 x 60) = 5400 s.
So, Coulombs = current (A) x 5400 s.
We know that 1 mole of aluminum requires 96,485 C of charge to deposit. Therefore, 0.056 mol of aluminum will require (0.056 x 96,485) C of charge.
Setting up the equation:
(0.056 x 96,485) = current (A) x 5400
Solving for current:
Current (A) = (0.056 x 96,485) / 5400 ≈ 1 A
Therefore, the current that must be passed into the solution of aluminum salt for 1 hour 30 minutes in order to deposit 1.5g of aluminum is approximately 1 Ampere.
Well, if you're trying to deposit aluminum, you're going to need an aluminum salt solution and some current to do the job. But hold on, let me do some calculations in my imaginary circus tent here...
First, let's convert the time into minutes. So, 1 hour is equal to 60 minutes, and we add another 30 minutes, which gives us a total of 90 minutes. Got it? Good!
Now, let's focus on the amount of aluminum you want to deposit, which is 1.5 grams. Since you mentioned that aluminum has an atomic mass of 27, we can calculate the number of moles of aluminum using the formula: moles = mass/molar mass.
In this case, moles = 1.5g / 27g/mol, which gives us approximately 0.056 moles of aluminum.
To deposit this much aluminum, we would need the same amount of electrons, as in a balanced chemical reaction, the number of moles of electrons is the same as the number of moles of the substance being deposited.
Now comes the tricky part. To calculate the current, we need to know the Faraday's constant, which is the charge of one mole of electrons. The Faraday's constant is approximately 96,485 Coulombs per mole.
Putting it all together, we can calculate the current using the formula: current = moles of electrons / time.
So, current = 0.056 moles / 90 minutes.
But please note that we need to convert minutes into seconds, as the unit for current is Coulombs per second.
So, current = 0.056 moles / (90 minutes * 60 seconds/minute).
And that's as far as we can go, my friend. Without knowing the specific value of time, we can't provide you with a precise current. But with these calculations, you should be able to figure it out!
And remember, if you need more help or just a good laugh, feel free to swing by my imaginary circus tent anytime!
To calculate the current required to deposit 1.5g of aluminum, 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 it.
The equation we can use to calculate the current is:
Mass (g) = (Current (A) * Time (s) * Atomic Mass (g/mol)) / (1 Faraday)
First, let's convert the time to seconds:
1 hour = 60 minutes
1 minute = 60 seconds
1 hour 30 minutes = (1 * 60 * 60) + (30 * 60) + 0 seconds
= 5400 + 1800 + 0
= 7200 seconds
Now, let's substitute the values into the equation:
1.5g = (Current (A) * 7200s * 27 g/mol) / (1 Faraday)
To calculate the current, rearrange the equation:
Current (A) = (1.5g * 1 Faraday) / (7200s * 27 g/mol)
Now, let's calculate the current:
Current (A) = (1.5 * 1) / (7200 * 27) ≈ 8.02 * 10^-6 A
Therefore, the current required to deposit 1.5g of aluminum in a solution of aluminum salt for 1 hour 30 minutes is approximately 8.02 microamperes (µA).
Coulombs needed = amperes x seconds
C = Amperes x 1.5 hours x 60 min/hr x 60 sec/min
We need C and we need amperes
We know that 96,485 coulombs will deposit 27/3 = 9 g Al metal. So how many C are necessary to deposit 1.5 g Al. That is
96,485 C x (1.5/9) = about 16,000 C. Then substitute into the above
16,000 = amperes x 1.5 hrs x (60 min/hr ) x (60 sec/min) and solve for amperes.
Post your work if you get stuck.