Consider the following standard electrode potentials: Ag*(aq) + e E→ Ag(s); E° = 0.80 V Mn2*(aq) + 2eE→ Mn(s); E° =-1.18 V Which of the following statements is false concerning the electrochemical cell given below? Mn(s) | Mn²*(aq) || Ag*(aq) | Ag(s) A) Under standard-state conditions, the cell potential is 1.98 V. B) The anode half-cell reaction is Mn(s) → Mn²*(ag) + 2e. C) The cell potential decreases with time. D) The reducing agent is Ag(s). E) The oxidizing agent is Ag*(aq).
Consider the following standard electrode potentials: Ag*(aq) + e E→ Ag(s); E° = 0.80 V Mn2*(aq) + 2eE→ Mn(s); E° =-1.18 V Which of the following statements is false concerning the electrochemical cell given below? Mn(s) | Mn²*(aq) || Ag*(aq) | Ag(s) A) Under standard-state conditions, the cell potential is 1.98 V. B) The anode half-cell reaction is Mn(s) → Mn²*(ag) + 2e. C) The cell potential decreases with time. D) The reducing agent is Ag(s). E) The oxidizing agent is Ag*(aq).
Chapter18: Introduction To Electrochemistry
Section: Chapter Questions
Problem 18.18QAP
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Consider the following standard electrode potentials:
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