How many moles of mercury will be produced by electrolyzing 1.0M Hg(NO3)2 solution with a current 2.00A for 2 hours.

To determine the moles of mercury produced through electrolysis, we need to use Faraday's Laws of Electrolysis.

Step 1: Calculate the total charge passed through the circuit.

Q = I * t

where Q is the charge in Coulombs (C), I is the current in Amperes (A), and t is the time in seconds (s).

Given that the current (I) is 2.00A and the time (t) is 2 hours (which is equivalent to 2 * 60 * 60 = 7200 seconds), we can substitute the values into the equation:

Q = 2.00A * 7200s = 14,400 C

Step 2: Calculate the moles of electrons passed through the circuit.

To calculate the moles of electrons (n), we can use the Faraday constant (F), which is 96485 C/mol.

n = Q / F

Substituting the values, we have:

n = 14,400 C / 96485 C/mol ≈ 0.1494 mol e-

Step 3: Determine the stoichiometry between electrons and mercury ions.

From the balanced equation:

Hg2+ + 2e- → Hg

We know that for every two electrons, one mole of mercury is produced.

Step 4: Calculate the moles of mercury produced.

moles of Hg = (moles of e-) / 2

moles of Hg = 0.1494 mol e- / 2 = 0.0747 mol Hg

Therefore, approximately 0.0747 moles of mercury will be produced by electrolyzing a 1.0 M Hg(NO3)2 solution with a current of 2.00 A for 2 hours.

To find the number of moles of mercury produced by electrolyzing the Hg(NO3)2 solution, we need to use Faraday's law of electrolysis.

Faraday's law of electrolysis states that the amount of substance produced or consumed during an electrolysis process is directly proportional to the quantity of electricity passed through the electrolyte.

The formula to calculate the amount of substance produced or consumed is:

n = (Q * Z) / (F),
where:
n is the number of moles of substance produced or consumed,
Q is the electrical charge in coulombs,
Z is the number of electrons transferred per molecule of substance, and
F is the Faraday constant, which is approximately 96,485 C/mol.

First, let's calculate the electrical charge passed through the electrolyte.

Given:
Current (I) = 2.00A (amperes),
Time (t) = 2 hours = 2 * 3600 seconds = 7200 seconds.

The electrical charge (Q) can be calculated using the formula:

Q = I * t.

Q = 2.00A * 7200s = 14400 C.

Next, we need to determine the value of Z, the number of electrons transferred per molecule of Hg(NO3)2. By examining the Hg(NO3)2 formula, we can see that there is one Hg atom per molecule, and Hg has a charge of 2+. Therefore, Z = 2.

Now, we can calculate the number of moles of mercury produced by using Faraday's law of electrolysis:

n = (Q * Z) / (F),
n = (14400 C * 2) / (96485 C/mol).

n = 0.298 mol (approximately).

Therefore, approximately 0.298 moles of mercury will be produced by electrolyzing the 1.0M Hg(NO3)2 solution with a current of 2.00A for 2 hours.

Mercury II? that is two electrons per atom.

charge=current*time=2C/sec*2*3600sec.
number electrons=charge*1/e

now it takes two electrons /atom
number atoms=numberelectrons/2
moles Hg= avag number/number atoms