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3) Which substance below is the strongest reducing agent? (a) Mg(s) (b) F2(g) (c) Cr(s) (d) K* (e) H2(g)

3) Which substance below is the strongest reducing agent? (a) Mg(s) (b) F2(g) (c) Cr(s) (d) K* (e) H2(g)

Chemistry
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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Please answer the question in the picture labeled #3. I also included a table of values im not sure if you will need it or if it will be irrelevant
DURABLE EW an Standar 3) Which substance below is the strongest reducing agent? (a) Mg(s) (b) F2(g) (c) Cr(s) (d) K* (e) H2(g)
Transcribed Image Text:DURABLE EW an Standar 3) Which substance below is the strongest reducing agent? (a) Mg(s) (b) F2(g) (c) Cr(s) (d) K* (e) H2(g)
TABLE 18.1 Standard Electrode Potentlals at 25 °C Reduction Half-Reaction F) + 2 e E (V) + 2F (aq) Stronger oxidizing agent H202(aq) + 2 H*(aq) + 2 e 2.87 +2 H20(0 → PBSO«(s) + 2 H20(1) → Mn02(s) + 2 H20() - Mn*(aq) + 4 H20(1) Weaker reducing agent PbO2(s) + 4 H*(ag) + SO,²¯(aq) + 2 e Mn04 (aq) + 4 H*(aq) + 3 e Mno. (aq) + 8 H*(aq) + 5 e Au+(aq) + 3e Pb02(s) + 4 H*(aq) + 2 e 1.78 1.69 1.68 1.51 - Au(s) 1.50 - Pb2*(aq) + 2 H20() → 2 cr (aq) 2 C*(aq) + 7 H2O) 2 H20(1) Mn+(aq) + 2 H,01) + (aq) + 3 H20() 1.46 Cl2lg) + 2 e Cr30, (aq) + 14 H*(aq) + 6 e 02(g) + 4 H*(aq) + 4 e MnO2(s) + 4 H*(aq) + 2 e 10, (aq) + 6 H*(aq) + 5 e Br() + 2 e Vo,"(aq) + 2 H*(aq) + e NO, (aq) + 4 H*(aq) + 3 e- 1.36 1.33 → 1.23 1.21 1.20 → 2 Br (aq) 1.09 - vo?"(aq) + H20() NOE) + 2 H20(1) → CIO, (aq) 1.00 0.96 CIO2() + e Ag"(aq) + e Fe*(aq) + e 0.95 Ag(s) + Fe?*(aq) 0.80 0.77 02(g) + 2 H*(aq) + 2 e Mno, (aq) +e b(s) + 2 e Cu*(aq) + e +H2O2(aq) 0.70 → Mn0,2 (aq) →21 (aq) → Cu(s) 4 OH (aq) + Cu(s) → H2SO3(aq) + H20(1) - Cu*(aq) - Sn*(aq) 0.56 0.54 0.52 02g) + 2 H20(1) + 4 e Cu*(aq) + 2 e 0.40 0.34 so, (aq) + 4 H*(aq) + 2 e Cu2*(aq) + e Snt(aq) + 2 e 2 H*(aq) + 2 e Fe(aq) + 3 e 0.20 0.16 0.15 - H2g) → Fe(s) → Pb(s) → Sn(s) -0.036 Pb2 (aq) + 2 e Sn2+(aq) + 2 e N2*(aq) + 2 e Cd*(aq) + 2 e Fe2+(aq) + 2 e Cr*(aq) + e Cr (aq) + 3 e Zn*(aq) + 2 e -0.13 -0.14 Ni(s) -0.23 → Cd(s) -0.40 - Fe(s) Cr2*(aq) -0.45 -0.50 - Cr(s) -0.73 + Zn(s) -0.76 + H2g) + 2 OH (aq) → Mn(s) + Al(s) -0.83 2 H20() + 2 e Mn2 (aq) + 2 e -1.18 -1.66 A*(aq) + 3 e Mg2+(aq) + 2 e Na (aq) + e Ca (aq) + 2 e Ba?+(aq) + 2 e K*(aq) + e oxidizing agent u*(aq) + e¯ -2.37 → Mg(s) → Na(s) -2.71 - Ca(s) -2.76 - Ba(s) -2.90 Stronger reducing agent - K(s) -2.92 Weaker - U(s) -3.04
Transcribed Image Text:TABLE 18.1 Standard Electrode Potentlals at 25 °C Reduction Half-Reaction F) + 2 e E (V) + 2F (aq) Stronger oxidizing agent H202(aq) + 2 H*(aq) + 2 e 2.87 +2 H20(0 → PBSO«(s) + 2 H20(1) → Mn02(s) + 2 H20() - Mn*(aq) + 4 H20(1) Weaker reducing agent PbO2(s) + 4 H*(ag) + SO,²¯(aq) + 2 e Mn04 (aq) + 4 H*(aq) + 3 e Mno. (aq) + 8 H*(aq) + 5 e Au+(aq) + 3e Pb02(s) + 4 H*(aq) + 2 e 1.78 1.69 1.68 1.51 - Au(s) 1.50 - Pb2*(aq) + 2 H20() → 2 cr (aq) 2 C*(aq) + 7 H2O) 2 H20(1) Mn+(aq) + 2 H,01) + (aq) + 3 H20() 1.46 Cl2lg) + 2 e Cr30, (aq) + 14 H*(aq) + 6 e 02(g) + 4 H*(aq) + 4 e MnO2(s) + 4 H*(aq) + 2 e 10, (aq) + 6 H*(aq) + 5 e Br() + 2 e Vo,"(aq) + 2 H*(aq) + e NO, (aq) + 4 H*(aq) + 3 e- 1.36 1.33 → 1.23 1.21 1.20 → 2 Br (aq) 1.09 - vo?"(aq) + H20() NOE) + 2 H20(1) → CIO, (aq) 1.00 0.96 CIO2() + e Ag"(aq) + e Fe*(aq) + e 0.95 Ag(s) + Fe?*(aq) 0.80 0.77 02(g) + 2 H*(aq) + 2 e Mno, (aq) +e b(s) + 2 e Cu*(aq) + e +H2O2(aq) 0.70 → Mn0,2 (aq) →21 (aq) → Cu(s) 4 OH (aq) + Cu(s) → H2SO3(aq) + H20(1) - Cu*(aq) - Sn*(aq) 0.56 0.54 0.52 02g) + 2 H20(1) + 4 e Cu*(aq) + 2 e 0.40 0.34 so, (aq) + 4 H*(aq) + 2 e Cu2*(aq) + e Snt(aq) + 2 e 2 H*(aq) + 2 e Fe(aq) + 3 e 0.20 0.16 0.15 - H2g) → Fe(s) → Pb(s) → Sn(s) -0.036 Pb2 (aq) + 2 e Sn2+(aq) + 2 e N2*(aq) + 2 e Cd*(aq) + 2 e Fe2+(aq) + 2 e Cr*(aq) + e Cr (aq) + 3 e Zn*(aq) + 2 e -0.13 -0.14 Ni(s) -0.23 → Cd(s) -0.40 - Fe(s) Cr2*(aq) -0.45 -0.50 - Cr(s) -0.73 + Zn(s) -0.76 + H2g) + 2 OH (aq) → Mn(s) + Al(s) -0.83 2 H20() + 2 e Mn2 (aq) + 2 e -1.18 -1.66 A*(aq) + 3 e Mg2+(aq) + 2 e Na (aq) + e Ca (aq) + 2 e Ba?+(aq) + 2 e K*(aq) + e oxidizing agent u*(aq) + e¯ -2.37 → Mg(s) → Na(s) -2.71 - Ca(s) -2.76 - Ba(s) -2.90 Stronger reducing agent - K(s) -2.92 Weaker - U(s) -3.04
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