Voltaic Cell Lab Experiment

Since electrons are negatively charged, their flow direction is from the reducing agents to oxidizing agents. In other words, the reducing agents release electrons and themselves get oxidized, while the oxidizing agents gain electrons, and themselves get reduced. The anode experiences oxidation, while the cathode experiences reduction. When redox reactions occur in a system where a wire separated the anode and cathode, electrons move would occur in that external wire that separated the anode and cathode, therefore, a current will flow (Neghmouche, 2007). A galvanic cell or primary cell is formed this way. Ag/Ag+//H+/H2 voltaic cell had been created. The voltmeter was turned on and observations recorded in the data table. The “OFF” button found on voltmeter was clicked to reset the virtual lab.

The following voltaic cells were set and observations recorded: • Ag/Ag+(aq)// H+/H2 (g) • Cu/Cu2++(aq)// H+/H2 (g) • H+/H2 (g)// Zn2+/Zn (s) • Cu/Cu2+(aq)//| Zn2+/Zn (s) • Ag/Ag+ (aq)// Zn2+/Zn (s) Observations For Ag/Ag+| | H+/H2, there was gray deposits of silver metal at the cathode. For Cu/Cu2+| | H+/H2, there was brown deposits of copper at the cathode. Volts 2. For Cu/Cu2+ | | H+/H2 Oxidation ½ -Reaction: H2 2H+ + 2e Eo anode = 0 Volts Reduction ½ -Reaction: Cu2+ + 2e Cu Eo cathode = 0. Volts Balanced Net Equation Cu2+ + H2 Cu + 2H+ E°cell = 0. V 3. For H2/H+ | | Zn2+/Zn Oxidation ½ -Reaction: Zn Zn2++ 2e Eo anode = -0. Volts Balanced Net Equation 2Ag+ + Zn 2Ag + Zn2+ E°cell = 0.

E°cell = 1. Volts Discussion Electrochemical reaction occurs in a voltaic cell and electrons are generated as electrodes form ions and as ions acquire electrons to form solids or gases. In a primary cell, the reduction and oxidation processes occur in an equilibrium such as an electrode gets into solution to form its ions and gets eaten away, the other electrode gets bigger due to deposits of its compound. Electrons are formed when an electrode dissolved into solution to form its ions. The electrode potentials for Ag/Ag+| | H+/H2, Cu/Cu2+| | H+/H2, and H+/H2| | Zn2+/Zn were obtained in this experiment. An ideal electrode potential is represented as below: E° cell = E° cathode - E° anode They were given in their standard reduction states.

According to this experiment, E° cell­­ for silver in respect to hydrogen was 0. V, that for copper in respect to hydrogen was 0. V, and that for zinc in respect to hydrogen was 0. Different metals must be used for there to be a potential difference. References Donne, S. W. General Principles of Electrochemistry. In Supercapacitors: Materials, Systems, and Applications.