How long, in seconds, would it take to deposit 10.5 g of copper onto an electrode from a solution of Cu2+ if a current of 2.00 A was applied?
Coulombs = amperes x seconds = ? You gave amperes; you need seconds.
You know 63.5/2 grams Cu (approx 32 g) will be deposited with 96,485 coulombs so
96,485 coulombs x (10.5/32) = approx 30000,
Note that my numbers are approx so you need to go through and refine ALL of them
Now you know total coulombs, so plug this number back into the first equation at the top and solve for seconds. Convert to minutes or hours if that is needed.
Post your work if you get stuck.
Well, aren't you sparking my interest with this electrifying question! To calculate the time it would take to deposit copper onto an electrode, we can use Faraday's law of electrolysis. The charge (Q) can be calculated by multiplying the current (I) by the time (t). The amount of copper that can be deposited onto the electrode is directly proportional to the charge, so we can determine the time it takes based on the amount of copper.
So, let's do the funky math! The charge (Q) can be calculated by multiplying the current (I) by the time (t). We need to rearrange the equation to solve for time.
Q = I * t
To deposit 10.5 g of copper, we need to find the corresponding charge. The atomic mass of copper is approximately 63.546 g/mol, so 10.5 g of copper is equal to:
10.5 g / (63.546 g/mol) = 0.1656 mol of copper
Each mole of electrons carries a charge of 96,485 C (aka 1 Faraday). Since copper has a charge of +2, we need to multiply the charge by 2 to account for the Cu2+ ions:
Charge (Q) = 0.1656 mol * 2 * 96,485 C/mol = 31,975.85 C
Now, let's substitute the given values into our equation and solve for time (t):
Q = I * t
31,975.85 C = 2.00 A * t
Dividing both sides by 2.00 A:
t = 31,975.85 C / 2.00 A
And now, let's calculate the time:
t ≈ 15,987.93 seconds
So, it would take approximately 15,987.93 seconds for 10.5 g of copper to be deposited onto an electrode when a current of 2.00 A is applied. Don't worry, you won't be waiting a shocking amount of time!
To calculate the time it would take to deposit 10.5 g of copper onto an electrode, we need to use Faraday's law of electrolysis. Faraday's law states that the amount of substance deposited (in grams) is directly proportional to the current (in amperes), time (in seconds), and the molar mass (in grams per mole) divided by the number of electrons transferred.
The molar mass of copper (Cu) is 63.55 g/mol, and it has a charge of +2 in the Cu2+ ion. Therefore, the number of electrons transferred is 2.
The equation to calculate the time is:
Time (in seconds) = (Mass (in grams) × 2) / (Current (in amperes) × Molar mass (in g/mol))
Substituting the given values:
Time = (10.5 g × 2) / (2.00 A × 63.55 g/mol)
Calculating the value:
Time = 21 g / (2.00 A × 63.55 g/mol)
Time = 21 / (2 × 63.55 s/mol)
Time = 0.165 s/mol
Therefore, it would take approximately 0.165 seconds to deposit 10.5 g of copper onto an electrode from a solution of Cu2+ when a current of 2.00 A is applied.
To determine the time it would take to deposit 10.5 g of copper onto an electrode, we need to use Faraday's law of electrolysis. This law states that the amount of substance deposited or released during electrolysis is directly proportional to the electric charge passed through the solution.
The formula to calculate the amount of substance deposited is:
Amount of substance (in moles) = Electric charge (in Coulombs) / Faraday's constant
First, we need to calculate the electric charge passed through the solution. The formula for calculating electric charge is:
Electric charge (in Coulombs) = current (in Amperes) × time (in seconds)
Given:
Current = 2.00 A
Amount of substance = 10.5 g
We need to find the time in seconds.
Now, we need to calculate the amount of substance in moles. The molar mass of copper can be found from the periodic table, which is approximately 63.55 g/mol. So, the number of moles of copper is:
Amount of substance (in moles) = 10.5 g / 63.55 g/mol
Next, we need to determine the electric charge by rearranging the formula:
Electric charge (in Coulombs) = Amount of substance (in moles) × Faraday's constant
The Faraday's constant is a physical constant representing the charge of 1 mole of electrons, which is equal to 96,485 Coulombs/mol.
Substituting the values into the formula, we get:
Electric charge (in Coulombs) = (10.5 g / 63.55 g/mol) × 96,485 Coulombs/mol
Now, we can substitute this value of electric charge into the previous formula and rearrange it to solve for time:
Time (in seconds) = Electric charge (in Coulombs) / current (in Amperes)
Substituting the values, we have:
Time (in seconds) = [(10.5 g / 63.55 g/mol) × 96,485 Coulombs/mol] / 2.00 A
Calculating this expression will give us the time required to deposit 10.5 g of copper onto the electrode from the given solution.