Lesson_25 - is deposited in the cathode(Notice that there...

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Lesson 25 Cell potentials and equilibrium constants What happens when a galvanic cell achieves equilibrium? Q nF RT E E cell cell ln 0 - = Nerst equation for non-equilibrium conditions: Nerst equation when chemical equilibrium is reached = - = RT nF E K K nF RT E cell c c cell 0 0 exp ln 0 Use this expression to calculate equilibrium constants using galvanic cells
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Lesson 25 Example 1
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Lesson 25 Example 2 Knowing that, 2+ - o Fe2+/Fe
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Lesson 25 Electrolysis If an opposing external potential causes the reaction in a galvanic cell to occur in the direction opposite to the spontaneous direction it is called electrolytic cell . Electrolytic cells uses electrical energy provided by an external circuit (a galvanic cell, for instance) to promote a chemical reaction that otherwise would not occur. E 0 Zn2+/Zn = -0.76 V E 0 Cu/Cu2+ = -0.34 V
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Lesson 25 Electrolysis Electrolytic cells can be used for the recovery of pure metals. In this electrolitic cell, the anode is impure Cu. Pure Cu
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Unformatted text preview: is deposited in the cathode. (Notice that there is no salt bridge.) Lesson 25 Electrolysis of water Pt Pt + NaOH O 2 H 2 2 H 2 O + 2 e-= H 2 + 2 OH-(cathode) 4 OH-= 2 H 2 O + O 2 + 4 e- (anode) 2 H 2 O = 2 H 2 + O 2 Lesson 25 Faraday’s law of electrolysis “The number of moles of material oxidized or reduced at an electrode is related by the stoichiometry of the electrode reaction to the amount of electricity passed through the cell.” Lesson 25 Example 3 Consider three electrolytic cells containing as Lesson 25 Example 4 If a concentrated NaCl solution is electrolized, 2 Lesson 25 Example 5 Electrolysis of an alkaline earth metal chloride using a current of 5.0 A for 748 seconds deposits 0.471 g of the metal at the cathode. What is the identity of the alkaline earth metal chloride. Lesson 25 Suggested readings...
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Lesson_25 - is deposited in the cathode(Notice that there...

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