An electrolysis cell for aluminum production operates at 5.0 V and a current of 1.5 x 10° A. Calculate the number of kilowatt-hours of energy required to produce 1 metric ton (1.0 x 10° kg) of aluminum. (1 kWh = 3.6 x 10° J and 1 J =1 C. V)Energy |kWhSubmit AnswerTry Another Version3 item attempts remaining

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Answered: An electrolysis cell for aluminum…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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O ELECTROCHEMISTRY = Using the Faraday constant 3/5 Suppose a current of 60. A flows through a copper wire for 35.0 minutes. Calculate how many moles of electrons travel through the wire. Be sure your answer has the correct unit symbol and round your answer to 2 significant digits. 0 μ Explanation Check 333 0 x10 DO X 00 S 5 ? Arvind V DEE do Ar
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Problem # 1 The fuel cell produces energy based on the reduction reaction of hydrogen, which in turn reacts with oxygen from air to produce water vapor. The reaction set is as follows: Net: H2 + ½ O2 → H2O What is the amount of hydrogen for the fuel cell to provide 500 watts of power with a total voltage of 48 V if it operates at 35% efficiency at full load? What is the amount of air required?
(Incorrect) In the electrolysis of aqueous KI, which substance is first produced at the anode? O₂ + 4H+ + 4e → 2 H₂O 1₂ +2e →21 2 H₂O +2 e → H₂ +2 OH K+ + e → K H₂ (Your answer) 12 (Correct answer) 02 K = 1.23 V = 0.53 V = -0.83 V = -2.93 V
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INTERACTIVE EXAMPLE Electroplating How long will it take to plate out 3.0 g Ni from aqueous Ni2+ with a current of 108.4 A? HOW DO WE GET THERE? Question Content Area How long will it take to plate out 3.0 g Ni with the 108.4 A current? ________s
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SIMULATION Voltaic Cells Under Standard Conditions Oxidizing Reducing Electrode EO °cathode -E°anode = E0 cell Agent Agent Potential (V) Au3+(aq) + 3e Au(s) +1.50 Br (t) + 2 e 2 Br (aq) +1.08 Cathode Anode Hg2+(aq) + 2 e Hg(t) +0.855 Ag*(aq) + e Ag(s) +0.80 Hg22 (aq) + 2 e 2 Hg(t) +0.789 Cu2*(aq) + 2 e Cu(s) +0.337 Sn (aq) + 2 e Sn2* (s) +0,15 2 H30*(aq) + 2 e H2(g) + 2 H20(s) 0.00 Sn2*(aq) + 2 e Sn(s) -0.14 Ni2*(aq) + 2 e Ni(s) -0.25 Cd2 (aq) + 2 e Cd(s) -0.40 Al3+ (aq) + 3 e Al(s) -1.66 Mg2+(aq) + 2 e Mg(s) -2.37 Li (aq) + e Li(s) -3.045 Click on an Oxidizing Agent and a Reducing Agent. What is the cell potential, E° cell, for the reaction? 2 Ag (aq) + Sn(s) → 2 Ag(s) + Sn²*(aq) 1 1 1 1 Gibbs Free Energy
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AGº for the following redox reaction. Round your answer to 4 significant digits. 2NO(g) +4H₂O (1)+3Zn² (aq) → 2NO3(aq) +8H* (aq) +3Zn(s) ☐ kJ Explanation Check G
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In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by electrolyzing brine, essentially an aqueous solution of sodium chloride. Suppose a current of 290. A is passed through an aqueous solution of NaCl for 20.0 seconds. Calculate the mass of pure chlorine produced. Be sure your answer has a unit symbol and the correct number of significant digits. Explanation Check 62022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center ere to search 99+ IA olo
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