A current of 1.5 A is passed for 2 hours through an aqueous solution of Pd X _ n where X is a monovalent anion. During the electrolysis process 2.977 g of Palladium metal gets deposited at the cathode. Calculate the charge on Pd ions. (Atomic mass of Pd =106.4 ~g / mol ).

Step-by-step solution

The total charge Q passed through the solution is given by Q = I t . Given I = 1.5 A and t = 2 hours = 2 3600 s = 7200 s. Q = 1.5 7200 = 10800 C. The number of moles of electrons passed is n_e = Q F = 10800 96500 0.1119 mol. The mass of Palladium deposited is m = 2.977 g and the atomic mass is M = 106.4 g/mol. The number of moles of Palladium deposited is n_ Pd = m M = 2.977 106.4 0.02798 mol. The reaction at the cathode is Pd ^ n+ + n e⁻ Pd . The stoichiometric ratio is n = n_e n_ Pd = 0.1119 0.02798 4 . Therefore