Can someone please explain how to tackle this problem?

Cu - Anode electrode
Zn - Cathode electrode

A current of 2 amps is sustained for 16 minutes. what mass of Cu(s) is deposited on the zinc electrode? (Faradays' constant: 96500 C/mol e-)

Coulombs = amperes x seconds.

C = 2 x 16 x 60 = 1,920
For every (63.55/2) g Cu plated it requires 96,500 C. So
(63.55/2) x (1920 C/96,500 C) = ?g Cu plated.

Thank you

Just one more question

Why is it (63.55/2) g Cu ?

To tackle this problem, you can use Faraday's law of electrolysis, which states that the mass of substance deposited or liberated at an electrode is directly proportional to the quantity of electric charge passed through the electrolyte solution.

Here's how you can approach the problem step by step:

1. Determine the quantity of electric charge.
The quantity of electric charge (Q) can be calculated using the formula:
Q = I * t
where I is the current (2 amps) and t is the time (16 minutes converted to seconds).

In this case, t is given in minutes, so you need to convert it to seconds before using it in the formula. One minute is equal to 60 seconds, so multiply 16 minutes by 60 to obtain the time in seconds.

2. Convert the quantity of electric charge to moles of electrons.
To convert the quantity of electric charge (Q) to moles of electrons, you need to divide it by Faraday's constant (F), which is 96500 C/mol e-

Moles of electrons = Q / F

3. Convert moles of electrons to moles of Cu.
According to the balanced equation for the electrochemical reaction, the same number of moles of electrons will correspond to the same number of moles of Cu deposited on the electrode.

4. Convert moles of Cu to mass.
To convert moles of Cu to mass, you need to use the molar mass of Cu, which is 63.55 g/mol. Multiply the number of moles of Cu by the molar mass to find the mass of Cu(s) deposited.

By following these steps, you can find the mass of Cu(s) deposited on the zinc electrode.