The main use of a Faraday is in the formula Q=nF. If this is rearranged, F=Q/n A Faraday is 96485 coulombs.
•96485 coulomb/mol of electrons (for J) •23054 C/mol (for Cal) •23.054 C/mol (for kCal) •
Coulomb is a unit of electric charge while Faraday is a unit of electric charge quantity present in one mole of electrons. One Coulomb is equal to one Faraday constant, which is approximately 96,485 coulombs.
The mathematical expression is Q = nF, where Q is the total charge in coulombs, n is the number of moles of electrons transferred (in this case, 3 moles for iron III sulfate to iron metal), and F is the Faraday constant (96,485 C/mol). Therefore, the number of coulombs necessary would be Q = 3 * 96485 C/mol = 289,455 C.
To calculate the grams of copper deposited during electrolysis, you need to use Faraday's law. First, calculate the total charge passed in coulombs by multiplying the current (7.50A) by the time (600 hours). Then, use the molar mass of copper to convert coulombs to grams. The molar mass of copper is 63.55 g/mol.
The equivalent weight of K2MnO4 is 158 g/mol. To calculate the produced KmnO4, we first determine the number of faradays in 96478 coulombs (1 F = 96485 C). Then we use the stoichiometry: 1 mol of K2MnO4 produces 1 mol of KMnO4. So, 158 g of K2MnO4 will produce 158 g of KMnO4.
To calculate the amount of copper deposited in coulombs, use the formula Q = It, where Q is the charge in coulombs, I is the current in amperes, and t is the time in seconds. Then, convert coulombs to grams of copper using the Faraday's constant (1 F = 96485 C/mol). Finally, calculate the mass of copper deposited.
Since 1 mole of neutral molecular hydrogen gas contains 2 moles of protons (H⁺) and 2 moles of electrons (e⁻), the total positive charge in 1 mole of neutral molecular hydrogen gas is equal to 2 moles of charge, or 2 faradays. This is equivalent to 2 x 96485 C = 192970 coulombs, or approximately 0.193 megacoulombs.
To determine the time required to produce 10.0 g of Bi, you would first calculate the number of moles of Bi needed using the molar mass of Bi. Then, use Faraday's constant (96,485 C/mol) to find the total charge (in Coulombs) needed to produce that amount of Bi. Finally, use the formula Q = It to calculate the time required, where Q is the charge in Coulombs, I is the current in amps, and t is the time in seconds.