To calculate the mass of copper deposited at the cathode, we can use Faraday's laws of electrolysis.

According to Faraday's first law, the amount of substance deposited at an electrode is directly proportional to the quantity of electric charge passed through the electrolyte.

The formula for calculating the mass of substance deposited is:
mass = (charge * molar mass) / (n * F)

Where:
mass = mass of substance deposited (in grams)
charge = quantity of electric charge passed through the electrolyte (in coulombs)
molar mass = molar mass of the substance (in grams/mole)
n = number of moles of electrons transfer per molecule of substance
F = Faraday's constant (96,485 coulombs/mole)

In this case, we want to calculate the mass of copper deposited at the cathode.

The molar mass of copper is 63.55 g/mol, and the number of moles of electrons transferred per copper ion is 2.
So, n = 2.

First, we need to calculate the quantity of electric charge (charge) using the formula:
charge = current * time

Given:
current = 5 amperes
time = 2 hours = 2 * 60 * 60 seconds = 7,200 seconds

So,
charge = 5 A * 7,200 s = 36,000 coulombs

Now, let's calculate the mass of copper deposited (mass):
mass = (charge * molar mass) / (n * F)
mass = (36,000 C * 63.55 g/mol) / (2 mol * 96,485 C/mol)
mass = 1.122 grams

Therefore, the mass of copper deposited at the cathode is 1.122 grams.

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