If a current of 5.0 Amps is passed through the electrolytic cell for .5 hour, how should you calculate the number of grams of bromine produced?
5.0 amps x 0.5 hr x 60 min/hr x 60 min/s = 9,000 coulombs.
2Br^- ==> Br2 + 2e
You know that 96,485 coulombs will form 1 equivalent of Br2 which is 159.8/2 = 79.9 g Br2.
You have 9,000 coulombs; therefore, how much Br2 will be formed?
79.9 x (9,000/96,485) = ?
To calculate the number of grams of bromine produced, you need to consider Faraday's law of electrolysis and the molar mass of bromine.
1. Determine the total charge passed through the electrolytic cell.
The charge (Q) can be calculated using the formula:
Q = I * t
where I is the current (5.0 Amps) and t is the time in hours (0.5 hours).
Q = 5.0 Amps * 0.5 hours = 2.5 Coulombs
2. Convert the charge to moles of electrons.
1 Faraday (F) is equal to 96,485 Coulombs of charge.
Since 1 mole of electrons is equal to 1 Faraday, the number of moles of electrons (n) can be calculated using the equation:
n = Q / F
n = 2.5 Coulombs / 96,485 Coulombs/mole = 2.59 x 10^-5 moles of electrons
3. Use the stoichiometry of the reaction to determine the moles of bromine produced.
The balanced equation for the production of bromine during electrolysis is:
2 Br^- → Br2 + 2 e^-
This means that for every 2 moles of electrons, 1 mole of bromine is produced.
Therefore, the moles of bromine produced (n_bromine) can be calculated using the equation:
n_bromine = 0.5 * n
n_bromine = 0.5 * 2.59 x 10^-5 moles = 1.30 x 10^-5 moles of bromine
4. Calculate the mass of bromine produced.
The molar mass of bromine (Br2) is 159.8 g/mol.
The mass of bromine (m_bromine) can be calculated using the equation:
m_bromine = n_bromine * molar mass
m_bromine = 1.30 x 10^-5 moles * 159.8 g/mol = 2.07 x 10^-3 grams of bromine
Therefore, approximately 2.07 x 10^-3 grams of bromine will be produced when a current of 5.0 Amps is passed through the electrolytic cell for 0.5 hour.
To calculate the number of grams of bromine produced in an electrolytic cell, you need to use Faraday's law and the molar mass of bromine.
Here are the steps to calculate it:
1. Start by finding the number of moles of electrons passed through the cell. This can be calculated using Faraday's law:
moles of electrons = (current in Amperes) * (time in seconds) / (Faraday's constant)
Faraday's constant is 96,485 Coulombs/mol of electrons.
In this case, the current is given as 5.0 Amps and the time is 0.5 hour, which is equal to 1800 seconds.
moles of electrons = (5.0 A) * (1800 s) / (96,485 C/mol)
2. Convert moles of electrons to moles of bromine. Since during the electrolysis of a compound, the moles of electrons are equal to the moles of the element being produced, the moles of electrons are also the moles of bromine.
3. Finally, convert moles of bromine to grams of bromine using the molar mass of bromine (79.904 g/mol).
Let's plug in the given values in the calculations:
moles of electrons = (5.0 A) * (1800 s) / (96,485 C/mol)
= 0.093 mol
moles of bromine = 0.093 mol
grams of bromine = 0.093 mol * 79.904 g/mol
= 7.431 g
Therefore, the number of grams of bromine produced in the electrolytic cell would be approximately 7.431 grams.