how long will it take for a 1.5A current to coat evenly a layer of copper 0.1mm thick on both sides of a 12cm by 12cm copper plate(e.c.e of copper is 0.000331gC; density of copper 9gcm?

the volume of Cu deposited is 12*12*0.01 = 1.44 cm^3

Thus, the mass of Cu is 1.44 * 9 = 12.96g
Now, how many moles of Cu is that? How many electrons needed?
See what you can do with that so far...

To find out how long it will take for a 1.5A current to coat evenly a layer of copper 0.1mm thick on both sides of a 12cm by 12cm copper plate, we can use Faraday's law of electrolysis.

1. First, we need to calculate the total amount of copper to be deposited on both sides of the plate. To do this, we use the formula:

Mass of copper = (Area × Thickness × Density) / (Equivalent weight of copper)

The equivalent weight of copper can be calculated using its atomic weight and the number of electrons involved in the reaction. The atomic weight of copper is 63.55 g/mol, and since the reaction involves the deposition of one copper ion (Cu2+) per two electrons, the equivalent weight of copper is 63.55 g/mol / 2 = 31.775 g.

Substituting the given values:

Mass of copper = (12 cm × 12 cm × 0.1 mm × 2 × 9 g/cm3) / (31.775 g)

2. Next, we calculate the total amount of charge required for the deposition of this mass of copper. The charge required can be calculated using the formula:

Charge = Mass of copper / Equivalent weight of copper

Substituting the previously calculated mass of copper:

Charge = (Mass of copper) / (Equivalent weight of copper)

3. To find the time taken for the deposition, we use Faraday's law, which states that the amount of charge passed is directly proportional to the time and the current. The formula is:

Q = I × t

Where:
Q = Charge
I = Current (1.5A)
t = Time

Rearranging the formula to solve for time:

t = Q / I

Substituting the previously calculated charge and current:

t = (Charge) / (Current)

By following these steps and substituting the provided values, you should be able to calculate the time it will take for the current to coat the copper plate evenly.

To determine how long it will take for a 1.5A current to coat a layer of copper evenly, we need to calculate the amount of copper that needs to be deposited and then divide it by the current.

First, calculate the total weight of copper that needs to be deposited:
Thickness of copper layer on one side = 0.1 mm
Total thickness of copper layer on both sides = 0.1 mm + 0.1 mm = 0.2 mm
Area of copper plate = 12 cm * 12 cm = 144 cm²
Volume of copper = thickness * area = 0.2 mm * 144 cm² = 28.8 cm³

Next, convert the volume of copper to mass using the density of copper:
Density of copper = 9 g/cm³
Mass of copper = volume * density = 28.8 cm³ * 9 g/cm³ = 259.2 g

Now, divide the mass of copper by the current to calculate the time:
Current = 1.5 A
Time = mass / current = 259.2 g / 1.5 A ≈ 172.8 seconds

Therefore, it will take approximately 172.8 seconds (or 2 minutes and 52.8 seconds) for a 1.5A current to evenly coat a layer of copper 0.1mm thick on both sides of a 12cm by 12cm copper plate.