Copper Metal was deposited at the cathode of an electrolytic cell from a solutio

Question

Copper Metal was deposited at the cathode of an electrolytic cell from a solution of Cu(NO3)2. The initial mass of the cathode was 16.4831 g and the final mass was 16.7569 g after 10.0 minutes using a current of 1.44 amperes.

A) Using this data, calculate an experimental value for Avagadro's Number.

B) Determine the accuracy of this experiment.

C) If the error in this experiment was determined to be from the ammeter, was it reading too high or too low? Explain/Show Reasoning

Please show all your steps if you would I have about 5 of these to do and I want to understand them.

Thanks

Explanation / Answer

Cu(s) -> Cu 2= + 2 e- ( 2 moles of e- )
Mass of Cu ( grams final - grams initial) = 16.7569 - 16.4831 = .2738 G of Cu (s)

mole of electrons = .2738g x 1mol cu/63.54g x 2mol of e/1 mol of Cu = .00861 moles of electrons
1 amp = 1 coulomb/sec

number of coulombs = 10 min x 60 sec/ 1 min x 1.44 c/sec = 864 Coulombs

the charge of one Electron = 1.60x10^-19 coulombs

number of electrons= 864 C x # of electron/ 1.60x10^-19 C = 5.4x10^21 eletrons

avagadro's number = number of e-/ mole of e-

= 5.4x10^21/ .00861 = 6.2x10^23

to determine the accuracy u need to compare the "actual" results vs. the " theorical"

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