Question

An inexpensive and accurate method of measuring the quantity of electricity flowing through a circuit is to pass the current through a solution of a metal ion and weigh the metal deposited. A silver electrode immersed in an Ag⁺ solution weighs 1.7854 g before the current has passed and weighs 1.8016 g after the current has passed. How many coulombs have passed?

Answer 1

Total of 127.013 C of charge is passed

Given

 weight of Ag solution before current has passed = 1.7854 g

  weight of Ag solution after current has passed = 1.8016 g

  Molecular mass of Ag = 107.86 g

  Faraday's Constant = 96485

First of all we have to apply Faraday's First Law of Electrolysis i.e

         m = ZQ

  where

Z is propotionality constant (g/C)

Q is charge (C)

Hence,

 Z = Atomic mass of substance/ Faraday's Constant

    = $\frac{107.86 g}{96485 C}$

    = 0.0011178 g/C

Now ,

   change in mass before and after the passing of current (Δm)

       Δm = 1.8016g-1.7854g

             =   0.0162g

    Now  amount of coulombs passed = $\frac{0.142g}{0.0011178 g/C }$

          amount of coulombs passed = 127.03524 C

Thus from the above conclusion we can say that amount of coulombs have passed is 127.03524 C

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