In an electrolysis experiment, a student used copper (Cu) electrodes and a Cu(NO3)2(aq) solution. The following data were collected: Time of reaction

6.55 minutes

Average current

3.752 A

Mass change of the cathode (g)

0.502 g increase

Molar mass of Cu

63.55 g/ mol

Write the half reaction for the electrochemical reaction that occurs at the cathode.
Calculate the number of Coulombs.
Calculate the number of moles of electrons transferred in this experiment. (4 pts)
If you were unable to calculate the Coulombs in Part b above, use 1663 C.
Calculate the moles of copper lost by the anode during the reaction. (4 pts) If you were unable to calculate the moles of electrons in Part c above, use 1.73 x 10-2 as the number of moles.
Calculate the molar mass of Cu.
Calculate the error for the calculated atomic mass. (2 pts) If you were unable to calculate the molar mass in Part e above, use 65.47 as the experimental molar mass of copper