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Exam 21: Electrochemistry: Chemical Change and Electrical Work

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Exam 1: Keys to the Study of Chemistry79 Questionsadd course
Exam 2: The Components of Matter105 Questionsadd course
Exam 3: Stoichiometry of Formulas and Equations87 Questionsadd course
Exam 4: The Major Classes of Chemical Reactions124 Questionsadd course
Exam 5: Gases and the Kinetic-Molecular Theory115 Questionsadd course
Exam 6: Thermochemistry: Energy Flow and Chemical Change85 Questionsadd course
Exam 7: Quantum Theory and Atomic Structure83 Questionsadd course
Exam 8: Electron Configuration and Chemical Periodicity85 Questionsadd course
Exam 9: Models of Chemical Bonding74 Questionsadd course
Exam 10: The Shapes of Molecules109 Questionsadd course
Exam 11: Theories of Covalent Bonding58 Questionsadd course
Exam 12: Intermolecular Forces: Liquids, Solids, and Phase Changes111 Questionsadd course
Exam 13: The Properties of Mixtures: Solutions and Colloids105 Questionsadd course
Exam 14: Periodic Patterns in the Main Group Elements: Bonding, Structure, and Reactivity118 Questionsadd course
Exam 15: Organic Compounds and the Atomic Properties of Carbon118 Questionsadd course
Exam 16: Kinetics: Rates and Mechanisms of Chemical Reactions88 Questionsadd course
Exam 17: Equilibrium: the Extent of Chemical Reactions104 Questionsadd course
Exam 18: Acid-Base Equilibria103 Questionsadd course
Exam 19: Ionic Equilibria in Aqueous Systems119 Questionsadd course
Exam 20: Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions94 Questionsadd course
Exam 21: Electrochemistry: Chemical Change and Electrical Work102 Questionsadd course
Exam 22: The Elements in Nature and Industry57 Questionsadd course
Exam 23: The Transition Elements and Their Coordination Compounds92 Questionsadd course
Exam 24: Nuclear Reactions and Their Applications94 Questionsadd course
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Consider the non-aqueous cell reaction 2Na(l) + FeCl2(s) Consider the non-aqueous cell reaction 2Na(l) + FeCl<sub>2</sub>(s) 2NaCl(s) + Fe(s) For which E°<sub>cell</sub> = 2.35 V at 200°C. <font face=symbol></font>G° at this temperature is 2NaCl(s) + Fe(s) For which E°cell = 2.35 V at 200°C. G° at this temperature is

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Question 101

The following half-reactions occur in the mercury battery used in calculators. If E°cell = 1.357 V, calculate the equilibrium constant for the cell reaction at 25°C. (Assume the stoichiometric coefficients in the cell reaction are all equal to 1.) HgO(s) + H2O(l) + 2e- The following half-reactions occur in the mercury battery used in calculators. If E°<sub>cel</sub><sub>l</sub> = 1.357 V, calculate the equilibrium constant for the cell reaction at 25°C. (Assume the stoichiometric coefficients in the cell reaction are all equal to 1.) HgO(s) + H<sub>2</sub>O(l) + 2e<sup>-</sup> Hg(l) + 2OH<sup>-</sup>(aq) ZnO(s) + H<sub>2</sub>O(l) + 2e<sup>-</sup> Zn(s) + 2OH<sup>-</sup>(aq) Hg(l) + 2OH-(aq) ZnO(s) + H2O(l) + 2e- The following half-reactions occur in the mercury battery used in calculators. If E°<sub>cel</sub><sub>l</sub> = 1.357 V, calculate the equilibrium constant for the cell reaction at 25°C. (Assume the stoichiometric coefficients in the cell reaction are all equal to 1.) HgO(s) + H<sub>2</sub>O(l) + 2e<sup>-</sup> Hg(l) + 2OH<sup>-</sup>(aq) ZnO(s) + H<sub>2</sub>O(l) + 2e<sup>-</sup> Zn(s) + 2OH<sup>-</sup>(aq) Zn(s) + 2OH-(aq)

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Question 102
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