Oxidation-reduction potential of the system BrO; +6H*/Br ¯+3H,O increases, incase of:H2SO4 additionTemperature decreasingNaNO3 additionKBr addition

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Answered: Oxidation-reduction potential of the…

Oxidation-reduction potential of the system BrO;¯+6H"/Br +3H2O increases, in case of: H,SO, addition Temperature decreasing NaNO3 addition KBr addition

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 table of standard electrode potentials Standard Electrode Potentials at 25 °C Reduction Half-Reaction E" (V) Au" (ag) + Зе Ag"(aq) + Fe* (aq) + 3e Sn²(aq) v*(aq) + 3e In"(ag) + 3e Eu" (ag) + 3e Cr* (aq) Тa" (ag) + Зе Zn*(aq) Nb* (aq) » Au(s) 1.50 e Ag(s) 0.80 » Fe(s) -0.04 + 2e » Sn(s) -0.14 » V(s) -0.26 » In(s) -0.34 » Eu(s) -0.35 + 3e » Cr(s) -0.42 » Ta(s) -0.60 » Zn(s) » Nb(s) → Ti(s) → Al(s) » Be(s) + 2e -0.76 + 3e -1.10 Ti (aq) + 2e Al" (aq) + 3e Ве (ag) + 2е Am* (ag) + 2e -1.63 -1.66 -1.85 » Am(s) -1.90 Pr* (ag) + 2e" » Pr(s) -2.00 Mg* (aq) + 20 - Mg(s) » Na(s) » Ca(s) -2.37 Na (aq) + Ca*(aq) Sr* (aq) + 2e Ba (aq) e -2.71 2e - 2.87 » Sr(s) -2.90 + 2e + Ba(s) -2.91
[References] Calculate the cell potential of a cell operating with the following reaction at 25°C in which Cr2 O,=0.025 M, I=0.035 M, [Cr]= 0.15 M, and H]= 0.30 M. Cr2 O, (ag) +61 (ag) + 14H (ag) -→ 20r (aq) + 312 (s) + 7H,0(1) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Standard Cathode (Reduction) Half-Reaction Potential, E (V) 0.54 L(s) +2e 21 (ag) Cr20, (ag) +14H" (ag) + 6e 2Cr (aq) +7H,0(1) 1.33 Cell potential = V
Using the provided standard reduction potentials, which of the following cells is an example of a Galvanic cell? A Au() Au"|| Ma* |Ma{e) ® Co(o) Co*| Fc*|Fo(e) B © Za(o)|Za*| cu*|cue)
Reduction potential of Mg2+ is -2.37 V. Reduction Potential of Fe2+ is 0.44 V. Based on the reaction below what is the electrical energy? Mg(s) + Fe2+(aq) + Fe(s) Fe2+(aq) = 0.18 M ; Mg2+(aq) = 0.53M
q19
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.
Use the following description of a galvanic cell to answer questions 4-7. One half-cell is prepared with a tin electrode submerged in 1.0 M Sn(NO,), and the other half-cell consists of a chromium electrode submerged in 1.o M Cr(NO), at standard temperature.
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…
A galvanic cell using Cu"/Cu and Cu?+/Cu was set up at 293 K and the non-standard cell potential was determined to be 0.175 V. Determine the concentration of ions in the cathode's solution if the concentration at the anode is 0.7787 M: (cathode)(M) number (rtol=0.03, atol=1e-08)
9:-0 electrode is called (a) anode, oxidation (b) anode, reduction O (c) cathode, oxidation (d) cathode, reduction (e) cannot tell unless we know the species being oxidized and reduced. The standard electrode potentials of the electrodes Cu+ | Cu and Ag+ | Ag are 0.337 V and 0.7991 V. What would be the concentration of Ag+ in a solution containing 0.06 M of Cu*+ ion such that both the metals can be deposited together. Assume that activity coefficients are unity and both silver and copper do not dissolve among themselves. 12.98x10-8 mole/dm-3 15.22x10-8 mole/dm-3 10.37x10-8 mole/dm-3 The standard electrode potentials of the electrodes Ag+ | Ag and Fe+, Fe* | Pt are 0.7991 V and 0.771 V respectively. Calculate the equilibrium constant for the reaction
The cell potential of the following cell is determined using an unspecified concentration of acid. What is [H*]given that the measured cell potential is -0.366 V and the anode reduction potential (E') is 0.222 V at 25°C? Agls) | AgCl(s) | CI(1.0 M) || H*(aq, ? M) | H2(g, 1.0 atm) | Pt(s) O 6.1x 102 M O 3.7 x 103M O 4.9x 105 M
Which redox reaction is spontaneous? OCr(s) + Al³+ (aq) → Cr** (aq) + Al(s) OPb(s) + Co²+ (aq) - Pb2+ (aq) + Co(s) OCu(s) + Zn²+ (aq) Cu²+ (aq) + Zn(s) -> O Mn(s) + Fe2+ (aq) - Mn²+ (aq) + Fe(s)