How many electrons would be required to deposit 6.35 ~g of copper at the cathode during the electrolysis of an aqueous solution of copper sulphate? (Atomic mass of copper =63.5 u , N _ A = Avogadro's constant):

Step-by-step solution

Cu Cu ⁺⁺+2 e ⁻ i.e, to deposit 1 mole of Cu at cathode from Cu ²⁺ SO ₄²⁻ solution =2 moles of electrons are required i.e, To deposit 6.35 ~g = 6.35 63.5 2= 2 10 = 1 5 moles Thus total no. of electrons required = N _ A 5