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Unformatted text preview: reaction? Assign a redox reaction to the relative location of the metals. Which metal will always be oxidized? Which metal will always be reduced? 6. Assign oxidation states, write the redox half-reactions, and label the oxidizing and reducing agent. a. Fe + CuSO 4 Cu + Fe 2 (SO 4 ) 3 b. Co + KMnO 4 CoO + KMnO 3 c. 2 H 2 + O 2 2 H 2 O 7. Draw a voltaic cell using Ag (s)/Ag + (aq) and Mg(s)/Mg 2+ (aq) as your electrodes and electrolytic solutions. Be sure to label: Anode and cathode (with charge) Flow of electrons Salt bridge Where oxidation occurs (and half reaction) Where reduction occurs (and half reaction) Provide the complete, balanced redox equation Calculate the voltage of the cell 8. Helpful neumonic devices and their meanings!...
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