Consider the following half-reactions: Half-reaction E° (V) Br2(1) + 2e → 2B1¯(aq) 1.080V Co2+(aq) + 2e → Co(s) -0.280V Cr3+(aq) + 3e Cr(s) -0.74OV (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Cr3+(aq) oxidize Br"(aq) to Br2(1)? no (6) Which species can be oxidized by Co2+(aq)? If none, leave box blank.

Consider the following half-reactions: Half-reaction E° (V) Br2(1) + 2e → 2B1¯(aq) 1.080V Co2+(aq) + 2e → Co(s) -0.280V Cr3+(aq) + 3e Cr(s) -0.74OV (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Cr3+(aq) oxidize Br"(aq) to Br2(1)? no (6) Which species can be oxidized by Co2+(aq)? If none, leave box blank.

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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Be sure to answer all parts. (a) Balance the skeleton reaction. Include the states of matter for each substance. (b) Calculate E (c) Determine whether the reaction is spontaneous. A table of standard electrode potentials is given below for reference. Cl₂(g) + Fe2+ (aq) → CI (aq) + Fe³+ (aq) (a) (b) (c) O Strength of oxidizing agent cell V not spontaneous spontaneous Selected Standard Electrode Potentials (298 K) Half-Reaction F2(g) + 2e7 Cl₂(g) + 2e7 MnO₂(s) + 4H+ (aq) + 2e7 NO3(aq) + 4H+ (aq) + 3e¯ Ag+ (aq) + e Fe³+ (aq) + e O₂(g) + 2H₂O() + 4e Cu²+ (aq) + 2e7 2H+ (aq) + 2e7 N₂(g) + 5H+ (aq) + 4e¯ Fe2+ (aq) + 2e7 2+ Zn²+ (aq) + 2e 2H₂O() +2e7 Na+ (aq) + e 2F (aq) 2C1 (aq) 2+ Mn²+ (aq) + 2H₂O(l) NO(g) + 2H₂O(l) Ag(s) Fe²+ (aq) 4OH(aq) Cu(s) H₂(g) N₂Hs+ (aq) Fe(s) Zn(s) H₂(g) + 2OH(aq) Na(s) Strength of reducing agent E half-cell (V) +2.87 +1.36 +1.23 +0.96 +0.80 +0.77 +0.40 +0.34 0.00 -0.23 -0.44 -0.76 -0.83 -2.71
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Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e → 2F*(aq) 2.870V Co2+*(aq) + 2e → Co(s) |-0.28OV 2+ Mg"(aq) + 2e → Mg(s) -2.37OV (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will Mg(s) reduce F2(g) to F"(aq)? (6) Which species can be reduced by Co(s)? If none, leave box blank.
is 0.085 correct or should it be 0.116? I got two answers and i’m not sure.
What is the voltage of the following cell? Use the Reduction Potential Table found in Chapter 17 notes. Cr(s)|Cr³*(0.25 M) || |2(s)|1-(0.20 M)|Pt(s)