Question

Average Current is 0.24 amps Total Charge given by integral plot is 130.5

Time(s) 600

Initial Mass of the copper electrode is 2.0296g

Initial mass of tin electrode is 0.7043g

Final mass of the copper electrode is 2.0797g

Final mass of the tin electrode is 0.4310g

Identify the anode and cathode.

Calculate the number of moles of tin plated onto the copper electrode using the delta m of the tin electrode then using delta m of the copper electrode:

Using the average current, calculate the total charge that flowed through the cell.

Using the current given by the integral, calculate the number of electrons that flowed through the cell.

Using the moles of tin and the number of electrons that flowed through the cell, calculate a value for Avogadro's number. Remember that each tin atom that reacted lost or gained two electrons.

Answer 1

Average current, i = 0.24 amp

Total charge, q = 130.5 C

Time, t = 600 s

Initial Mass of the copper electrode = 2.0296g

Initial mass of tin electrode = 0.7043g

Final mass of the copper electrode = 2.0797g

Final mass of the tin electrode = 0.4310g

Since the tin is deposited onto the copper electrode, this means tin is oxidized at the anode.

Anode is Tin electrode and Cathode is Copper electrode.

Mass of tin plated onto the copper electrode = 0.7043 - 0.4310

= 0.2733 grams

Atomic mass of tin = 118.71 g/mol

Moles of tin plated onto the copper electrode = 0.2733 / 118.71

= 0.0023 moles

We know that:

i = q / t

q = i * t

= 0.24 * 600

= 144 Coulombs

Charge on an electron = 1.602 x 10^-19 coulombs

Number of electrons = 144 / (1.602 x 10^-19)

= 8.98 x 10²⁰ electrons

Since 1 tin atom loses 2 electrons

Number of tin atoms involved = 8.98 x 10²⁰ / 2

= 4.49 x 10²⁰ atoms

Avogadro's number = Atoms / Moles

= 4.49 x 10²⁰ / 0.0023

= 1.95 x 10²³