Lawrie Ryan and Roger Norris Solutions for Chapter: Electrochemistry, Exercise 7: Questions

A learner passed a constant electric current of $0.15 \mathrm{A}$ through a solution of silver nitrate, using pure silver electrodes, for $45 \min$ exactly. The mass of the anode decreased by $0.45 \mathrm{g}$. Use this data to calculate the charge on a mole of electrons. (A_r value: $\left[\mathrm{Ag}\right] = 108$)

An accurate value of the Faraday constant is $96485 \mathrm{C} {\mathrm{mol}}^{-1}$. An accurate value for the charge on one electron is $1.6022 \times {10}^{-19} \mathrm{C}$. Use these values to calculate a value of the Avogadro constant to $5$ significant figures.