Quantitative Electrolysis

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.

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: $\left[\mathrm{Ag}\right] = 108$)

Calculate the volume of oxygen produced at r.t.p. when a concentrated aqueous solution of sodium sulfate is electrolysed for $55.0 \min$ using a current of $0.70 \mathrm{A}$. ($\mathrm{F}= 96500 \mathrm{C} {\mathrm{mol}}^{-1}$; $1 \mathrm{mole}$ of gas occupies $24.0 {\mathrm{dm}}^3$ at r.t.p.) (Write the value only rounded off to two decimal places)

Calculate the volume of hydrogen produced at r.t.p. when a concentrated aqueous solution of sulfuric acid is electrolysed for $15.0 \min$ using a current of $1.40 \mathrm{A}$. ($\mathrm{F}= 96500 \mathrm{C} {\mathrm{mol}}^{-1}$; $1 \mathrm{mole}$ of gas occupies $24.0 {\mathrm{dm}}^3$ at r.t.p.) (Write the value only rounded off to two decimal places)