Consider the following half-reactions. Cl2(g) + 2 e– → 2 Cl–(aq) E° = +1.36 V Ag+(aq) + e– → Ag(s) E° = +0.80 V Cu2+(aq) + 2 e– → Cu(s) E° = +0.34 V Sn2+(aq) + 2 e– → Sn(s) E° = –0.14 V Al3+(aq) + 3 e– → Al(s) E° = –1.66 V Which of the following species will reduce Cu2+(aq) ion? Ag(s) and Sn^2+(aq) Cl^-(aq) and Ag(s) Cl2(g) and Ag^+(aq) Sn(s) and Al(s) Sn^2+(aq) and Al^3+(aq)
Consider the following half-reactions. Cl2(g) + 2 e– → 2 Cl–(aq) E° = +1.36 V Ag+(aq) + e– → Ag(s) E° = +0.80 V Cu2+(aq) + 2 e– → Cu(s) E° = +0.34 V Sn2+(aq) + 2 e– → Sn(s) E° = –0.14 V Al3+(aq) + 3 e– → Al(s) E° = –1.66 V Which of the following species will reduce Cu2+(aq) ion? Ag(s) and Sn^2+(aq) Cl^-(aq) and Ag(s) Cl2(g) and Ag^+(aq) Sn(s) and Al(s) Sn^2+(aq) and Al^3+(aq)
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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Consider the following half-reactions.
Cl2(g) + 2 e– → 2 Cl–(aq) | E° = +1.36 V | |
Ag+(aq) + e– → Ag(s) | E° = +0.80 V | |
Cu2+(aq) + 2 e– → Cu(s) | E° = +0.34 V | |
Sn2+(aq) + 2 e– → Sn(s) | E° = –0.14 V | |
Al3+(aq) + 3 e– → Al(s) | E° = –1.66 V |
Which of the following species will reduce Cu2+(aq) ion?
Ag(s) and Sn^2+(aq)
Cl^-(aq) and Ag(s)
Cl2(g) and Ag^+(aq)
Sn(s) and Al(s)
Sn^2+(aq) and Al^3+(aq)
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