Answer to Question #281670 in Inorganic Chemistry for jeonnn

Question

An aqueous solution of a platinum salt is electrolyzed at a current of 2.498 A

for 3.00 h. As a result, 9.09 g of metallic Pt are formed at the cathode.

Following this half reaction: Ptn+ + ne- → Pt, calculate the charge (represented

by “n+” on the half reaction) on the Pt ions in this solution.

Answer 1

m = (M x I x t) / (n x F)

n = (M x I x t) / (m x F) = (195,084 g/mol x 2.498 A x 10800 s) / (9.09 g x 96485 C/mol) = 6

The charge +6