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1. A sodium sulfate solution was electrolyzed using inert Pt electrodes. The cathode reaction was: 2 H2 0 + 2 e - → H2 + 2 OH-. If a current of 3.0 amp was used for 30 min, what weight of H2 gas would be produced? 2. What volume of H2 gas at STP would be produced during the passage of 30,000 Coul in the electrolysis of H2 O? 3. Give the notation for a cell that utilizes the reaction: a) Cl2 (g) + 2 I – (aq) → 2 Cl – (aq) + I2 (s) b) What is the E° for the cell? c) Which electrode is the cathode? 4. The standard electrode potential for the Fe2+ ↔ Fe3+ + e – half reaction is -0.770 V. a) Using the Nernst equation [ E = E°− ( 0.059/n) log [Oxid]/[Red]] calculate the voltage of this half-cell when the [Fe3+] is 1.0 x 10 -3 and [Fe2+] is 1.0 x 10 -1. b) Calculate the approximate equilibrium constant (K) for the half reaction.
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