Table 20.2 Half-reaction E° (V) Cr3+ (aq) + 3e--Cr(s) Fe2+ (aq) + 2e -Fe (s) Fe3+ (aq) + e-Fe2+ (s) Sn+ (aq) + -0.74 -0.440 +0.771 + 2e- - Sn2+ (aq) +0.154 Error correction: Note the third line in the table should read: Fe3+ (ag) + e¯ --> Fe2+ (ag) Which of the following reactions will occur spontaneously as written? O a. Sn 4+ 2+ (ag) + Fe (s) Sn 2+ (aq) + Fe (s) Ob. 2Cr (s) + 3Fe 2+ (s)→ 3Fe (s) + 2Cr 3+ (aq) 3+ 2+ 4+ (ag) + 2Cr (s) C. 2Cr (aq) – 3Sn (aq)+3Sn 2+ d. 3Fe (aq) + Cr 3+ (ag) – Cr (s) + 3Fe 3+ (aq)

Table 20.2 Half-reaction E° (V) Cr3+ (aq) + 3e--Cr(s) Fe2+ (aq) + 2e -Fe (s) Fe3+ (aq) + e-Fe2+ (s) Sn+ (aq) + -0.74 -0.440 +0.771 + 2e- - Sn2+ (aq) +0.154 Error correction: Note the third line in the table should read: Fe3+ (ag) + e¯ --> Fe2+ (ag) Which of the following reactions will occur spontaneously as written? O a. Sn 4+ 2+ (ag) + Fe (s) Sn 2+ (aq) + Fe (s) Ob. 2Cr (s) + 3Fe 2+ (s)→ 3Fe (s) + 2Cr 3+ (aq) 3+ 2+ 4+ (ag) + 2Cr (s) C. 2Cr (aq) – 3Sn (aq)+3Sn 2+ d. 3Fe (aq) + Cr 3+ (ag) – Cr (s) + 3Fe 3+ (aq)

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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Table 20.2 Half-reaction Ee (V) Cr3+ (aq) + 3e- ¬ Cr (s) -0.74 Fe2+ (aq) + 2e- - Fe (s) -0.440 Fe3+ (aq) + e- ¬ Fe2+ (s) +0.771 Sn4+ (aq) + 2e- - Sn2+ (aq) +0.154 ?Which of the following reactions will occur spontaneously as written Sn4+ (aq) + Fe2+ (aq) – Sn2+ (aq) + Fe (s) .a 3FE2+ (aq) - Fe (s) + 2Fe3+ (aq) .b O 3Fe (s) + 2Cr3+ (aq) - 2Cr (s) + 3FE2+ (aq) .c O 3Sn4+ (aq) + 2Cr (s) - 2Cr3+ (aq) + 3Sn2+ (aq) .d O Sn4+ (aq) + Fe3+ (aq) - Sn2+ (aq) + Fe2+ (aq) .e O
What is the standard reduction potential of Mg2+ --> Mg if the standard reduction potential of Zn2+ --> Zn is -0.76 V? Mg/ Mg2+ (aq) // Zn²+ (aq) / Zn E = +1.61 V -0.85 V +0.85 V +2.37 V -2.37 V none of the above
What is the correct shorthand notation for the cell on the previous slide? Oxidation: Ag(s) Ag*(aq) + e- Reduction: Mno,(s) + 4 H*(ag) + 2 e - Mn2+(aq) + 2 H,0() A. Ag(s) | Ag*(aq) || H*(aq), Mn²*(aq), H20() | MnOg(s) В. Ag*(aq) | Ag(e) || Mn02(a) | Mn²*(aq), H20(). H*(aq) C. Mno2(3) | H*(aq), Mn²*(aq), H20() || Ag*(aq) | Ag(3) D. Mn2*(aq). H20(). H*(@q) | MnO2(s) || Ag(3) | Ag*(aq)
Consider the following half-reactions: Half-reaction E° (V) Ag+(aq) + e- Ag(s) 0.799V Ni2+(aq) + 2e- Ni(s) -0.250V 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)? (yes/no) (6) Which species can be reduced by Ni(s)? If none, leave box blank.
Determine the equilibrium constant at 255 K for the following reaction under acidic conditions. 4H+ (aq) + MnO₂ (s) + 2Fe²+ (aq) Mn²+ (aq) + 2Fe³+ (aq) + 2H₂O(1) The two half-reactions are: MnO₂ (s) + 4H+ (aq) + 2e¯ Fe³+ (aq) + e¯ Mn²+ (aq) + 2H₂O(1) Eº = 1.23 V Fe²+ (aq) E° = 0.770 V
Item 1 < 1 of 25 Constants | Periodic Table Part A The standard cell potential (E') of the reaction below is -0.55 V. The value of A G for the reaction is J/mol. I2 (5) + 2Br (aq) → 21 (aq) + Brz (1) O 1.1- 105 O 0.54 O 0.55 O 5.5 - 106 O none of the above Submit Request Answer
Considering the reaction and the information in the Excel table below, what should be entered into cell D3 to calculate Kc? Fe3+(aq) + 2 SCN (aq) = Fe(SCN),"(aq) (bp).2( A 1 Equilibrium Concentration (M) B 2 Fe3+ SCN Fe(SCN)2+ Equilibrium Constant 3 9.70E-04 1.70E-04 2.60E-05 =C3/(A3*B3^2) O =C3/(A3^2*B3) O =A3*B3^2/C3 O =C3/(A3*B3)^2 O =C3/(A3*B3)
Consider the following half-reactions: Half-reaction E° (V) Hg2+(aq) + 2e- Hg(l) 0.855V Pb2+(aq) + 2e- Pb(s) -0.126V Mn2+(aq) + 2e- Mn(s) -1.180V (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 Mn2+(aq) oxidize Hg(l) to Hg2+(aq)? (yes / no) (6) Which species can be reduced by Pb(s)? If none, leave box blank.
Consider the following half-reactions: Half-reaction E° (V) Br2(l) + 2e- 2Br-(aq) 1.080V Sn2+(aq) + 2e- Sn(s) -0.140V Al3+(aq) + 3e- Al(s) -1.660V (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(l) oxidize Al(s) to Al3+(aq)? (yes/no) (6) Which species can be reduced by Sn(s)?
Which redox reactions occur spontaneously in the forward direction? Check all that apply. Pb(s) + Mg2+ (aq)- > Pb2+ ( aq) + Mg(s) Ni(s) + Pb2+ (aq)-> Ni2+ (aq) + Pb(s) Ni(s) + Zn2+ (aq) - > Ni2+ (aq) + Zn(s) Cr(s) + 3Ag+(aq) - > Cr 3+ (aq) + 3Ag(s)
Half-Reaction E° (V) 2H* (aq) + 2e¯ - H2 (9) 0.000 Ag* (aq) + e¯ → Ag (s) 0.7996 2H20 (I) + 2e¯ - H2 (g) + 20OH" (aq) -0.8277 AI3+ (aq) + 3e¯ → Al (s) -1.676 H2O2 (aq) + 2H* (aq) + 2e¯ → 2H20 (1I) 1.776 Au+ (aq) + e¯→ Au (s) 1.692 I2 (s) + 2e¯ → 21¯ (aq) 0.5355 Au3+ (aq) + 3e¯ → Au (s) 1.498 2103- (aq) + 12H* (aq) + 10e¯ → I2 (s) + 6H2O (1) Mg2+ (aq) + 2e - Mg (s) 1.195 Ba2+ (aq) + 2e¯ → Ba (s) -2.912 -2.372 Br2 (1) + 2e¯ → 2B1¯ (aq) 1.066 Mn2+ (aq) + 2e" → Mn (s) -1.185 Ca2+ (aq) + 2e¯ → Ca (s) -2.868 Mno2 (s) + 4H+ (aq) + 2e¯ → Mn2+ (aq) + 2H20 (1) 1.224 Cl2 (g) + 2e¯ → 2C1- (aq) 1.35827 Mno4- (aq) + 8H* (aq) + 5e¯ → Mn2+ (aq) + 4H2O (1) 1.507 Co2+ (aq) + 2e¯ → Co (s) -0.28 Mnog- (aq) + 2H20 (I) + 3e¯ → MnO2 (s) + 40H¯ (aq) 0.595 Co3+ (aq) + e¯ → Co2+ (aq) 1.92 HNO2 (aq) + H+ (aq) + e¯ → NO (g) + H2O (I) 0.983 Cr2+ (aq) + 2e¯ → Cr (s) -0.913 N2 (g) + 4H2O (1) + 4e¯ → 40H" (aq) + N2H4 (aq) -1.16 Cr3+ (aq) + 3e¯ → Cr (s) -0.744 NO3- (aq) + 4H* (aq) + 3e¯ → NO (g) + 2H2O (1) 0.957 Cr3+…
Consider the following half-reactions: Half-reaction E° (V) Br2(l) + 2e- 2Br-(aq) 1.080V Pb2+(aq) + 2e- Pb(s) -0.126V Fe2+(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 Fe2+(aq) oxidize Br-(aq) to Br2(l)? (yes/no) (6) Which species can be oxidized by Pb2+(aq)?