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What is a faraday?
The main use of a Faraday is in the formula Q=nF. If this is rearranged, F=Q/n A Faraday is 96485 coulombs.
What is faraday constant?
•96485 coulomb/mol of electrons (for J) •23054 C/mol (for Cal) •23.054 C/mol (for kCal) •
What is the different between Coulomb and Faraday?
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.
What mathematical expression identifies the number of coulombs necessary to produce one mole of iron metal from an aqueous solution of iron III sulfate?
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.
How many grams of copper would be deposited during electrolysis of copper salt by a current of 7.50A for 600 hours?
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
In manufacture of potassium permanganate by electrolysis of k2mno4 what should be the equivalent weight of kmno4 how much kmno4 will be produced by 96478 coulombs or one farady?
Equivalent weight of KMnO4 is equal with molar weight of KMnO4. The some is and for K2MnO4, K2MnO4 - e +OH- --------- KMnO4 + KOH In general, Equivalent weight = Molar weight / Number of electrons that take or give one molecule Equivalent weight of KMnO4 = Molar weight of KMnO4 / 1
How much copper is deposited if a current of 0.2 amps is passed for 2 hours through a copper II sulphate solution?
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.
How many megacoulombs of positive charge are in 1 mole of neutral molecular hydrogen gas?
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.
The electrolysis of BiO plus produces pure bismuth How long would it take to produce 10.0 g of Bi by the electrolysis of a BiO plus solution using a current of 25.0 amps?
Farady's Equation for his Law of Electrolysis applies. The law states "The mass of a substance altered at an electrode during electrolysis is directly proportional to the quantity of electricity transferred at that electrode. Quantity of electricity refers to the quantity of electrical charge, typically measured in coulomb." The equation is m = (Q/F)*(M/z) where m is the mass of material, Q is the total charge passed through the electrode, F is the Faraday constant (equal to the charge of 1 mole of electrons), M is the molar mass of the substance and z is the charge on the ion to be reduced. From elementary circuit theory, we know the Q = I*t. That is to say the current the for a given current Q passed through a point for a given time t, the total charge is know. Substitute I*t for Q and solve for t: t = mFz/IM The Faraday constant F is 96485 Coulombs/mol The Molar Mass of Bismuth, M, is 208.9804 grams/mol m is given as 10g I is given as 25amps (25 Coulombs/mol) We still need z. The oxidation state of oxygen is almost always O2-. So in BiO+, Bi will be Bi3+. Therefor, z = 3. t = (10g * 96485C/mol * 3) / (25C/sec * 208.9804 g/mol) t = 554.0328 sec or 550 sec This answer assumes 100% efficiency in your apparatus and 100% yield, which will never, ever happen.
