Unit 7: Redox Cell Potentials.

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Presentation transcript:

Unit 7: Redox Cell Potentials

What is going on in the Copper Lab? What did you observe at the pencil that was connected to the red + terminal? Orange/brown stuff collected on the pencil What did you observe at the pencil that was connected to the black - terminal? Bubbles, smell of chlorine.

The Electrochemical Cell Source: www.battterybot.com Source: http://www.reuk.co.uk Alkaline Battery Lead-Acid (car) Battery

The Electrochemical Cell The species being oxidized LOSES electrons Occurs at the anode (both start with vowels!) Is the reducing agent Is the more active metal Will go from metal to ion, thus putting out electrons

The Electrochemical Cell The species being reduced GAINS electrons Occurs at the cathode (both start with consonants!) Is the oxidizing agent Is the less active metal Will go from ion to metal, thus taking in electrons

The Electrochemical Cell Cu2+ + Zn → Zn2+ + Cu Copper Zinc CuSO4 ZnSO4 Write the oxidation half-reaction Write the reduction half-reaction What is the oxidizing agent? What is the reducing agent? Where is the cathode? Where is the anode? Image: http://commons.wikimedia.org/wiki/File:Galvanic_cell_unlabeled.svg

The Electrochemical Cell Cu2+ + Zn → Zn2+ + Cu Write the oxidation half-reaction Write the reduction half-reaction What is the oxidizing agent? What is the reducing agent? Where is the cathode? Where is the anode?

The Electrochemical Cell Cu2+ + Zn → Zn2+ + Cu Copper Zinc CuSO4 ZnSO4 How can we determine the voltage (the cell potential) created by an electrochemical cell? Electrons flow from anode to cathode. We can measure this. Image: http://commons.wikimedia.org/wiki/File:Galvanic_cell_unlabeled.svg

Determining Cell Potentials Write the oxidation and reduction half-reactions Use the standard reduction table to determine: Ecell = Eoreduction + Eooxidation *Remember to flip the sign if you flip the half-reaction!

Cell Potential Example Determine the standard reduction potentials and say if the reaction is spontaneous as written: Mn2+ + 4H2O + Sn2+ → MnO4- + 8H+ + Sn