Consider the following half-reactions:Half-reactionE° (V)2+Hg"(aq) + 2e→ Hg(1) 0.855VCo**(aq) + 2e → Co(s) -0.280V2+Fe"(aq) + 2e→ Fe(s) |-0.440v(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 Hg*(aq) oxidize Fe(s) to Fe2*(aq)?|(6) Which species can be oxidized by Co2*(aq)?If none, leave box blank.

The solutions are given below -

Answered: Consider the following half-reactions:…

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
Consider the following half-reactions: Half-reaction E° (V) Ag*(aq) + e" Co2*(aq) + 2e → Ag(s) 0.799V → Co(s) |-0.280V Zn2*(aq) + 2e → Zn(s) -0.763V (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 Zn2*(aq) oxidize Ag(s) to Ag"(aq)? (6) Which species can be reduced by Co(s)? If none, leave box blank.
R = 8.314 mol·K F = 96,485 mot AG = AG° + RT · In(Q) ΔΕΔΕ-).In(O) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e¯ → 2 H20 (1) 1.229 2 z" (aq) Z2 (s) + 2 e 3+ (aq) + 3 е 0.426 A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e H2 (g) + 2 OH (aq) - 0.828 G (s) - 1.245 > M2+ (aq) + 2 e - 1.893 → M (s) A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. Consider the same cell from the above prompt. Calculate AG° in kJ/mol for this galvanic cell. Report your answer with 4 significant figures. You do not need to report units with your answer. If your value is negative, make sure to include a "-" symbol.
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.
Consider the following half-reactions: Half-reaction E° (V) |Cl2(g) + 2e¯ → 2C1 (aq) 1.360V Co2+(aq) + 2e Mn2+(aq) + 2e → Co(s) -0.280V → Mn(s)-1.180V (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 CI"(aq) reduce Mn2+(aq) to Mn(s)? (6) Which species can be reduced by Co(s)? If none, leave box blank.
Complete and balance the following half-reaction in acidic solution. Be sure to include the proper phases for all species within the reaction. S2O3² (aq) → S4O6²¯(aq) 1 + 4- 2 Reset 0₂ H OH- ų 3 ( ) 0²- 4 e S 5 6 05 ☐6 1L (s) H+ 2+ H₂O 8 18 4+ x H₂O 0 ☐ ☐o (1) (g) (aq) H3O+ Delete

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