0:00Time Left:1:55:37Miguel Zapata: Attempt 1Question 28 (3.333333333 points)Determine the potential of the following galvanic cell: Ga(s) I Ga3+(aq) |I Ag*(aq) IAg(s)Ag*(aq) + e" → Ag(s) Eº = 0.7994 VGa3+(aq) + 3e → Ga(s) Eº = -0.530 V-0.269 V1.33 V0.269 V2.98 V-1.33 VIl app.honorlock.comYour screen.Stop sharingHideGuard888F4FBF10%&45YUFJKVMOSISOcommandVCOB

Because, the standard reduction potential value (E0) of Ga is more negative that is -0.530 V than Ag…

Determine the potential of the following galvanic cell: Ga(s) I Ga*(aq) II Ag*(aq) I Ag(s) Ag*(aq) + e" → Ag(s) Eº = 0.7994 V Ga3+(aq) + 3e → Ga(s) Eº = -0.530 V -0.269 V 1.33 V 0.269 V O 2.98 V -1.33 V

Determine the potential of the following galvanic cell: Ga(s) I Ga(aq) II Ag(aq) I Ag(s) Ag*(aq) + e" → Ag(s) Eº = 0.7994 V Ga3+(aq) + 3e → Ga(s) Eº = -0.530 V -0.269 V 1.33 V 0.269 V O 2.98 V -1.33 V

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Chapter1: Chemical Foundations

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Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

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