The amount of electricity required to produce 12.7 g of copper from CuSO4 using inert electrode would be [Atomic mass of Cu

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1. To find:

   The amount of electricity required to produce 12.7 g of copper from [tex]CuSO_{4}[/tex] using inert electrode.

   Calculation:

   First, let’s write the half cell reaction:

   [tex]Cu^{+2}+2e^{-}\rightarrow Cu[/tex]

   Now, from the equation:

   • 2F (or 2 moles of electron) is required to get 1 mole (or 63.5 gram) of Copper.

   So, amount of electricity needed for 12.7 grams of Copper is:

   [tex] = \dfrac{2}{63.5} \times 12.7[/tex]

   [tex] = 0.4 \: F[/tex]

   So, amount of electricity needed is 0.4 Faraday (or 0.4 moles of electrons).

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