96485 expressed in scientific notation is 9.6485X10^4.
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.
Assume it is a copper 2 salt and no side reactions it would require 96485 x 2 coulombs of charge per mole of copper or per 63.5 g of copper. 1 coulomb is 1 amp.second so 7.5 x 600 x 3600 x 63.5 / (96485 x 2) g = 5331 g Cu
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.