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How much electricity in term of Faraday is required to produce 40 gram of Al from Al2O3 ? (Atomic mass of Al = 27 g/mol?
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How much electricity in term of Faraday is required to produce 40 gram...
Al3++3e−→Al


1 mole (27 g) of Al will require 3 moles of electrons.
40 g of Al will require 273×40F​=4.4 F
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How much electricity in term of Faraday is required to produce 40 gram...
Calculation of Electricity Required to Produce 40g of Al from Al2O3


Step 1: Write the Balanced Equation


The first step is to write a balanced chemical equation for the reaction that takes place during the production of aluminium from aluminium oxide.


2Al2O3(s) → 4Al(l) + 3O2(g)


Step 2: Determine the Number of Moles of Al2O3


The next step is to determine the number of moles of aluminium oxide required to produce 40 grams of aluminium. We can do this by using the atomic mass of aluminium and the molar mass of aluminium oxide.


Molar mass of Al2O3 = (2 x 27) + (3 x 16) = 102 g/mol


Number of moles of Al2O3 = Mass of Al2O3 / Molar mass of Al2O3


Number of moles of Al2O3 = 40 / 102 = 0.3922 moles


Step 3: Determine the Number of Moles of Al


From the balanced chemical equation, we know that 4 moles of aluminium are produced for every 2 moles of aluminium oxide consumed.


Number of moles of Al = 4 x 0.3922 / 2 = 0.7844 moles


Step 4: Calculate the Quantity of Charge Required


The quantity of charge required to produce a certain amount of aluminium can be calculated using Faraday's laws of electrolysis. Faraday's laws state that the amount of product produced at an electrode is directly proportional to the quantity of electricity passed through the electrolyte.


The quantity of charge required to produce one mole of aluminium can be calculated using the equation:


Q = n x F


where Q is the quantity of charge in coulombs, n is the number of moles of aluminium produced, and F is the Faraday constant, which is equal to 96,485 coulombs per mole of electrons.


Q = 0.7844 x 96,485 = 75,702 coulombs


Step 5: Convert Coulombs to Amperes and Time


The quantity of charge required to produce the aluminium can be converted into amperes and time using the equation:


Q = I x t


where I is the current in amperes and t is the time in seconds.


I = Q / t


t = Q / I


Assuming a current of 1 ampere, the time required to produce the aluminium can be calculated as follows:


t = 75,702 / 1 = 75,702 seconds


This is equivalent to:


t = 75,702 / 3600 = 21 hours and 1 minute


Step 6: Answer the Question


The quantity of electricity required to
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How much electricity in term of Faraday is required to produce 40 gram of Al from Al2O3 ? (Atomic mass of Al = 27 g/mol?
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