Calculate the total Charge in coulombs (C) that passed through the electrolytic

Question

Calculate the total Charge in coulombs (C) that passed through the electrolytic cell for each trial Use your answer from 1 above to calculate the number of electrons in the e electrolysis for each trial. Recall from the famous Millikan oil-drop experiment that the charge of an electron is 1.602 times 10^-19 coulombs per electron Determine the number of copper atoms lost from the anode each the Remember that the electrolysis process uses two electrons to produce one copper ion (Cu^2) Calculate the number of cocker atoms per gram of copper lost at the anode for each trial The mass test at the anode is equal to both the mass of copper atoms lost and the mass of copper ions produced (the mass of the electrons is negligible) Calculate the number of copper atoms in a mole of copper for each trial Compare this value to Avogadro's number

Explanation / Answer

(1)

C=It=0.468*180=84.24 C

(2)

1 C=6.24*1018 electrone

So no of electrones=84.24*6.24*1018=5.258*1019 electrones

(3)

Number of Cu2+ ions = 1/2 number of electrons measured

Number of Cu2+ ions = (5.258 *1019electrons)(1 Cu2+ /2 electrons)
Number of Cu2+ ions = 2.62*10 19 Cu2+ ions

(4)

2.62*10 19 Cu2+ ions/0.0027 gm =9.7378*1021 Cu atom/gm

(5)

Cu atoms/mole of Cu = (9.7378x 1021 copper atoms/g copper) *63.546 gm/mol (MW of Cu)
Cu atoms/mole of Cu = 6.187 x 1023 copper atoms/mole of copper

Avogadro no=6.022*1023 atoms/mole

So it is approximately same.

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