How many moles of mercury will be produced by electrolysis 1 m hg (no3)^2 solution with a current of 2A for 3 hours. Hg (no3)^2=200.6
You must mean 1 M and not 1 m. m stands for molality. M stands for molarity.
Coulombs = Amperes x seconds = 2A x 3 h x (60 min/hr) x (60 sec/min) = approx 7200 C.
Then you know 96,485 C will deposit 1/2 mol Hg so
0.5 mol Hg x 7200 C/96,485 C = ? mol Hg Hg.
To calculate the number of moles of mercury (Hg) produced by electrolysis, we can use Faraday's law of electrolysis.
First, calculate the charge (Q) using the formula:
Q = I * t
where I is the current (2A) and t is the time (3 hours). Be sure to convert the time from hours to seconds by multiplying by 3600.
Q = 2A * 3 hours * 3600 seconds/hour = 21,600 coulombs
Next, calculate the number of moles (n) of electrons involved in the electrolysis using Faraday's constant (F), which is 96,485 coulombs/mole.
n = Q / F
n = 21,600 coulombs / 96,485 coulombs/mole = 0.224 moles of electrons
Since the balanced equation for the electrolysis of Hg(NO3)2 is:
Hg(NO3)2(aq) -> Hg(l) + 2NO2(g) + O2(g)
We can see from the equation that for every 2 moles of electrons, 1 mole of mercury is produced. Thus, the number of moles of mercury produced is half the number of moles of electrons.
Therefore, the number of moles of mercury produced is:
0.224 moles of electrons * (1 mole of Hg / 2 moles of electrons) = 0.112 moles of Hg
Lastly, since you provided the molar mass of Hg(NO3)2, which is 200.6 g/mol, we can calculate the mass of mercury produced:
Mass of Hg = Number of moles * Molar mass
Mass of Hg = 0.112 moles * 200.6 g/mol = 22.47 grams (rounded to two decimal places)
So, the amount of mercury produced by electrolysis is approximately 22.47 grams.
To find the number of moles of mercury produced by electrolysis, we can use Faraday's laws of electrolysis.
First, let's determine the total charge passed through the electrolytic cell.
We know the current (I) is 2A, and the time (t) is 3 hours. However, we need to convert the time from hours to seconds, as the SI unit for time in the equations is seconds.
1 hour = 3600 seconds
So, 3 hours = 3 * 3600 = 10,800 seconds.
The total charge (Q) is given by the formula:
Q = I * t
Q = 2A * 10,800s
Q = 21,600 C (Coulombs)
Now, we need to determine the number of moles of electrons (n) that passed through the cell. This can be done using Faraday's constant (F), which represents the charge of one mole of electrons (1 Faraday = 96,485 C):
n = Q / F
n = 21,600 C / 96,485 C/mol
n ≈ 0.2238 moles of electrons
Since the stoichiometry of the electrolysis reaction is 1 mole of mercury produced per 2 moles of electrons, we can determine the number of moles of mercury (nHg):
nHg = 0.2238 moles of electrons / 2
nHg ≈ 0.1119 moles of mercury
Therefore, approximately 0.1119 moles of mercury will be produced by electrolysis.