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Electrolysis

e-. e-. e-. e-. Electrochemistry. Electrolysis. Chapter 17 Section 7. e-. e-. e-. e-. Electrochemistry – Electrolytic Cells. EXO. ENDO. A galvanic cell produces current spontaneous. positive cell potential

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Electrolysis

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  1. e- e- e- e- Electrochemistry Electrolysis Chapter 17 Section 7

  2. e- e- e- e- Electrochemistry – Electrolytic Cells EXO ENDO A galvanic cell produces current spontaneous. positive cell potential An electrolytic cell uses energy to produce a chemical changenegative cell potential. Forcing a current through a cell cell potential is negative Electrical work causes a non spontaneous reaction to occur. Practice uses - recharging batteries producing aluminum plating to prevent corrosion p. 792

  3. e- e- e- e- Electrochemistry – Electrolytic Cells Since the electrical work causes e- to flow in the opposite direction the anode and cathode are reversed. e- flow from anode to cathode The salt bridge ion flow is opposite in the two cells Galvanic Cell Electrolytic Cell p. 817

  4. e- e- all about negative charge, electrons about any charge negative or positive 1.60222 x 10-19 C 6.022 x 1023 mol • e- e- e- Electrochemistry – Quantitative Electrochemistry Stoichiometry and Electrochemistry How much (g, mole, atoms) chemical change occurs with the flow of a given current (amps) for a specific time (seconds, minutes, hours)? Amps = unit of charge = 1 coulomb / 1 second 1 mole of e- = the charge of a 1 faraday= 96485 coulomb / 1 mol e- The faraday is derived from the charge of an electron in coulombs and the number of e- in a mole. The faraday connects electricity to stoichiometry.

  5. e- e- e- e- Electrochemistry – Quantitative Electrochemistry E = cell potential (volts) Amp = 1 C / 1 sec Volt = 1 J / 1 C Watt = 1 J / 1 second Volts x Amp = Watt (power) kWh = kilowatts x hours 1kWh = 3.6 x 106 J

  6. e- e- e- e- Electrochemistry- Sample Page 816-817 How much copper is plated out when 10.0 amps is applied for 30 minutes to the Zn ǀ Zn2+ ǁ Cu2+ ǀ Cu cell at standard conditions?

  7. e- e- e- e- Electrochemistry- Sample 17.9 Page 818 How long must a current of 5.00 A be applied to a solution of Ag+ to produce 10.5 g of solid silver?

  8. e- e- e- e- Electrochemistry- Sample Page 819 • Plating out for metals = reducing • So the metal with the highest reduction potential would plate out first Which would plate out first?

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