How much copper would be plated by a current of 1.5 A in a time of 1.0 h?
an ampere is a Coulomb per second
there are 6.242E18 electrons in a Coulomb
moles of electrons = (6.242E18 * 1.5 * 60 * 60) / 6.02E23
it takes two electrons to plate a Cu atom
find the moles of electrons
... divide by two to find the moles of Cu
multiply by the molar mass of Cu to find the grams
To find out how much copper would be plated, we can use Faraday's law of electrolysis.
The formula is:
m = (I * t * M) / (n * F)
Where:
m = mass of the substance plated (in grams)
I = current (in amperes)
t = time (in seconds)
M = molar mass of the substance (in grams/mol)
n = number of electrons transferred in the reaction
F = Faraday's constant (approximately 96,485 C/mol)
In this case, we need to calculate the mass of copper plated (m), so we can rewrite the formula as:
m = (I * t * M) / (2 * F)
First, let's convert the time from hours to seconds:
t = 1.0 h * 60 min/h * 60 s/min
t = 3600 s
The molar mass of copper (Cu) is approximately 63.55 g/mol.
Now, let's calculate the mass of copper plated:
m = (1.5 A * 3600 s * 63.55 g/mol) / (2 * 96485 C/mol)
m ≈ 0.884 g
Therefore, approximately 0.884 grams of copper would be plated by a current of 1.5 A in a time of 1.0 hour.
To calculate the amount of copper plated by a current, you need to use Faraday's law of electrolysis. According to Faraday's law, the amount of substance (copper in this case) that is deposited or plated on an electrode is directly proportional to the amount of charge passing through the circuit.
The formula to calculate the amount of substance plated is given by:
Amount of substance plated = (Current × Time) / Faraday's Constant
Step 1: Identify the current value and time given in the question.
Given:
Current (I) = 1.5 A (Amperes)
Time (t) = 1.0 h (hours)
Step 2: Convert the time to seconds since Faraday's Constant uses seconds as the unit of time.
1 hour is equal to 3600 seconds, so:
Time (t) = 1.0 h = 1.0 × 3600 seconds = 3600 seconds
Step 3: Determine the value of Faraday's Constant.
Faraday's Constant (F) is a constant that represents the charge of one mole of electrons and is approximately equal to 96485 Coulombs per mole.
Step 4: Calculate the amount of substance plated using the formula.
Amount of substance plated = (Current × Time) / Faraday's Constant
Amount of substance plated = (1.5 A × 3600 s) / 96485 C/mol
Now, you can calculate the amount of copper plated by substituting the given values into the formula:
Amount of substance plated = (1.5 A × 3600 s) / 96485 C/mol
Calculating this expression will give you the amount (in moles) of copper plated by the given current in the given time.