Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e¯ –→ 2F"(aq) 2.870V 2H*(aq) + 2e H2(g) 0.000V |APt(aq) + Зe Al(s) -1.660V (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 Al(s) reduce F2(g) to F(aq)? (6) Which species can be oxidized by H*(aq)? If none, leave box blank.

Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e¯ –→ 2F"(aq) 2.870V 2H(aq) + 2e H2(g) 0.000V |APt(aq) + Зe Al(s) -1.660V (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 Al(s) reduce F2(g) to F(aq)? (6) Which species can be oxidized by H(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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Consider the following half-reactions: Half-reaction E° (V) 2(s) + 2e → 21(aq) l0.535V Sn*(ag) + 2e Sn(s)l-0.140V Fe"(aq) + 2e → Fe(s) -0.440V (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 I(aq) reduce Fe"(aq) to Fe(s)? (6) Which species can be oxidized by Sn2*(aq)? If none, leave box blank.
(19) sa len Consider the following redox reaction that occurs in a voltaic cell: Cr2+ (aq) + Cu²+ (aq) → Cr³+ (aq) + Cu+ (aq) If the cell is operating at 25°C, what is the value of the equilibrium constant (Kea)? (A) 1.41 x 10¹¹ (B) 1.19 x 1018 (C) 5.53 x 105 (D) 2.79 x 1033 (E) 1.81 x 10-6 11020 ucleus of calcium-39 captures one
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.
Use the References to access important values if needed for this question. Consider the following half-reactions: Half-reaction E° (V) Hg*(aq) + 2e → Hg(1) 0.855V Co2*(ag) + 2e → Co(s) -0.280V Mg-*(aq) + 2e → Mg(s)|-2.370V (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 Hg²+(aq) oxidize Mg(s) to Mg?*(aq)?| (6) Which species can be oxidized by Co2*(aq)? If none, leave box blank. (Previous Next
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 ° (V) Br2(1) + 2e → 2Br°(aq) |1.080V Sn²+ (aq) + 2e . Sn(s) |-0.140V 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 Br2(0) oxidize Zn(s) to Zn2*(aq)? (6) Which species can be oxidized by Sn2*(aq)? If none, leave box blank.
Consider the following galvanic cell: Cu(s) | Cu²+ (aq) || Ag+(aq) | Ag(s) Identify the cathode and state if it is being oxidized or reduced (please refer to chart on reference data page.) (A) Cu is the cathode; it is being oxidized (B) Cu is the cathode; it is being reduced (C) Ag is the cathode; it is being oxidized (D) Ag is the cathode; it is being reduced (E) Since the E values for both Ag and Cu are positive, they are both cathodes and being reduced
Use the References to access important values if needed for this question. Consider the following half-reactions: Half-reaction E° (V) I2(s) + 2e → 21(aq) 0.535V *(aq) + 2e" → Ni(s) |-0.250V Mg"(aq) + 2e"- Mg(s)-2.370V (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 Mg*(aq) oxidize I'(aq) to I,(s)? (6) Which species can be oxidized by Ni²* If none, leave box blank. (aq)?
Consider the following half-reactions: Half-reaction E° (V) Hg-"(aq) + 2e" Hg(1) 0.855V 2+, Pb2*(aq) + 2e → Pb(s)-0.126V Zn*(aq) + 2e" – Zn(s) -0.763V (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 Zn(s) reduce Hg*"(aq) to Hg(1? (6) Which species can be reduced by Pb(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.
5. A more complex example where other atoms are involved. Balance the following reaction in basic solution. r (aq) + MnO4 (aq) MnO, (s)+ BrO;" (aq) TABLE 19.1 Standard Electrode Potentials at 25 °C Reduction Half-Reaction E'(V) F + 20 H,0,(aq) + 2 H(aq)+2 e 2F(aq) 2.87 Stronger oxidizing agent Weaker 2 H,0 - PBSO (s) +2 H,0) -Mn0(s)+ 2 H,0) Mn (aq) 4 H,O) - Auts) 1.78 reducing agent PO,(s) + 4 H"(ag) + S0,2-(aq) + 2 e 1.69 Mno, (aq)+ 4 H'(aq) 3 e Mno, (aa) + 8 H (aq)+5 e Au (aq)+3e PbO,(s)+ 4 H(aa) + 2 e Cl,(g) + 2 e" 1.68 1.51 1.50 1.46 - P (ag) + 2 HO - 2a(aq) 1.36 1.33 Cr0, (aq) + 14 H'(ag) + 6 e 0+ 4 H (aq) + 4 e MnO(s)+4 H'(aq) +2 e 10, (aq) 6 H'(aq) + 5e Br+2e vo, (aq) + 2 H'(aq) + e NO, (aq) + 4 H°(aq) + 3e CIO+e 2 C"(aq) + 7 H,On - 2 H,O1) 1.23 Mn (aq) + 2 HyOV) 121 ulae) + 3 H,0() 2 Br (ag) - vo"(aq) +H,00 - NO + 2 H,O0 - CIO, (aa) - Agis) 1.20 1.09 1.00 0.96 0.95 Ag"(aa) + e 0.80 Fe (aq) + O+2 H'(aq)+2e - Fe*(aq) 0.77 - H,O,(ag) 0.70 Mn0, Taa) + e Mn0 (aa) 0.56 8) + 2 e…
Consider the following half-reactions: (1) The weakest oxidizing agent is: (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)? | + Half-reaction F₂(g) + 2e 2H+(aq) + 2e™ Mg2+ (aq) + 2e™ (6) Which species can be reduced by H₂(g)?| If none, leave box blank. E° (V) 2.870V H₂(g) 0.000V Mg(s) -2.370V 2F (aq) enter formula