For numbers 2 and 3, refer to the following half-reactions and standard potentials. E° (V) K* + e K Mg2+ + 2e Mg Cd2+ + 2e - Cd -2.92 -2.37 -0.40 Aut + e → Au +1.68 2. Which is the strongest reducing agent among those shown above? * Cd Mg K Au 3. Which of the following reactions will occur spontaneously? * O Mg2 + Cd Mg + Cd2+ Au + K* Aut + K Mg + 2K Mg2+ + 2K 2AU* + Mg - 2Au + Mg2 O O

For numbers 2 and 3, refer to the following half-reactions and standard potentials. E° (V) K* + e K Mg2+ + 2e Mg Cd2+ + 2e - Cd -2.92 -2.37 -0.40 Aut + e → Au +1.68 2. Which is the strongest reducing agent among those shown above? * Cd Mg K Au 3. Which of the following reactions will occur spontaneously? * O Mg2 + Cd Mg + Cd2+ Au + K* Aut + K Mg + 2K Mg2+ + 2K 2AU* + Mg - 2Au + Mg2 O O

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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Refer to the galvanic cell below (the contents of each half-cell are written beneath each compartment): V Pt 0.10 M MnO4 0.40 М Cr3+ 0.20 M Mn2+ 0.30 M Cr,0,2- 0.010 M H* 0.010 MH* The standard reduction potentials are as follows: MnO, + 8H* + 5e → Mn2+ + 4H,O, ɛ° = 1.51 V Cr,0,2- + 14H* + 6e 2Cr** + 7H2O, ɛ° = 1.33 V When current is allowed to flow, which species is oxidized? O Cr,0,²- Cr³+ MnO4 Mn2+ O H*
Given the standard electrode reduction potentials, which reaction will occur spontaneously?
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Which of these half-reactions contains the strongest reducing agent at standard conditions? Pb2*(aq) + 2e¯ → Pb(s); E° = 0.13 V Cd2*(aq) + 2e- → Cd(s); E° = - 0.40 V Cu2+(aq) + 2e¯ → Cu(s); E° = 0.34 V
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6. Sketch a voltaic cell for the following overall redox reaction. 3 Cl2(g) + 2 Fe(s) — 6 CІ (аq) + 2 Fe3+(aq) а. Label the anode and cathode b. Indicate the half-reaction occurring at each electrode c. Indicate the species present in each solution.
Consider the following two half-reactions and their standard reduction potentials. N2(g) +H,0(1) E° = 1.766 V MnO, (s) + 2H,0(1) E° = 1.673 V N,0(g) + 2H*(aq) + 2e¯ → MnO,(aq) + 4H*(aq)+3e¯ 1st attempt l See Calculate E°for the spontaneous redox reaction that occurs when these two half-reactions are coupled. V