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7) If an electrochemical reaction is spontaneous, a) cell potential is negative, and the more electronegative metal is the anode (oxidized) b) cell potential is negative, and the more electronegative metal is the cathode (reduced) c) cell potential is positive, and the more electronegative metal is the anode (oxidized) d) cell potential is positive, and the more electronegative metal is the cathode (reduced)

7) If an electrochemical reaction is spontaneous, a) cell potential is negative, and the more electronegative metal is the anode (oxidized) b) cell potential is negative, and the more electronegative metal is the cathode (reduced) c) cell potential is positive, and the more electronegative metal is the anode (oxidized) d) cell potential is positive, and the more electronegative metal is the cathode (reduced)

Chemistry
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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**Electrochemistry Questions** **7) If an electrochemical reaction is spontaneous:** a) cell potential is negative, and the more electronegative metal is the anode (oxidized) b) cell potential is negative, and the more electronegative metal is the cathode (reduced) c) cell potential is positive, and the more electronegative metal is the anode (oxidized) d) cell potential is positive, and the more electronegative metal is the cathode (reduced) **8) Given the choice among Cu, Al, Fe, Ag, Sn, and Zn to create an electrochemical cell with the greatest standard potential, which two metals would you choose and why?** a) Zn and Al, they are the two highest in the table b) Cu and Ag, they are the two lowest in the table c) Sn and Fe, they are in the center of the table d) Al and Ag, they are the most far apart in the table **9) What is the standard cell potential of a Mg and Ag electrochemical cell? (The reaction is spontaneous.)** a) 3.17 V b) -3.17 V c) 1.57 V d) -1.57 V **10) Which is the oxidation half reaction for a Mg and Ag electrochemical cell? (The reaction is spontaneous.)** a) \( \text{Mg}^{2+} + 2e^- \rightarrow \text{Mg(s)} \) (Mg gains electrons) b) \( \text{Mg(s)} \rightarrow \text{Mg}^{2+} + 2e^- \) (Mg loses electrons) c) \( \text{Ag}^+ + e^- \rightarrow \text{Ag(s)} \) (Ag gains electrons) d) \( \text{Ag(s)} \rightarrow \text{Ag}^+ + e^- \) (Ag loses electrons)
Transcribed Image Text:**Electrochemistry Questions** **7) If an electrochemical reaction is spontaneous:** a) cell potential is negative, and the more electronegative metal is the anode (oxidized) b) cell potential is negative, and the more electronegative metal is the cathode (reduced) c) cell potential is positive, and the more electronegative metal is the anode (oxidized) d) cell potential is positive, and the more electronegative metal is the cathode (reduced) **8) Given the choice among Cu, Al, Fe, Ag, Sn, and Zn to create an electrochemical cell with the greatest standard potential, which two metals would you choose and why?** a) Zn and Al, they are the two highest in the table b) Cu and Ag, they are the two lowest in the table c) Sn and Fe, they are in the center of the table d) Al and Ag, they are the most far apart in the table **9) What is the standard cell potential of a Mg and Ag electrochemical cell? (The reaction is spontaneous.)** a) 3.17 V b) -3.17 V c) 1.57 V d) -1.57 V **10) Which is the oxidation half reaction for a Mg and Ag electrochemical cell? (The reaction is spontaneous.)** a) \( \text{Mg}^{2+} + 2e^- \rightarrow \text{Mg(s)} \) (Mg gains electrons) b) \( \text{Mg(s)} \rightarrow \text{Mg}^{2+} + 2e^- \) (Mg loses electrons) c) \( \text{Ag}^+ + e^- \rightarrow \text{Ag(s)} \) (Ag gains electrons) d) \( \text{Ag(s)} \rightarrow \text{Ag}^+ + e^- \) (Ag loses electrons)
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