Using this table of standard reduction potentials determine which ofthe following is the strongest reducing agent.Hall ReonRall &107A+-A"0401.99Coe + 281.7NAga +eA a50++ S0, + ROCCe0.2POO + S0 e , 20LS+ HD6041.311.50NhPARO, + S soL4-0.2)a. 2 20C1313Ma + 4T M HO1.21LO9Za ZaLO0Mr+2Me-LANONO+ 280-230.91-237A AgNe-231077Ca+-290-22K KMO+ Mao,G.54O AGCIO Fe+O Cu²-Stop sharII Proctorio is sharing your screen.O Ag

We know that Reducing agent : Reducing agent is defined as the substance that reduces other…

Using this table of standard reduction potentials determine which of the following is the strongest reducing agent. Hall Reon Nall 020 040 A+-A" 1.99 Aga+ Ag a 50++ S0, + RO 1.7N 0.22 C Ce PO Ot + S0 e AS, 20 189 M HO 1.51 As -Aa NO N LO a. 2 20 1.50 L4 Sa+- Se Nh N PARO, + S so -4.2) 1.3 13 .21 Ma + 4T M HO 10 4 • O LO9 Za Za LO0 Ma + Me NO NO + 280 -23 -237 -I7 -231 -2% -20 2 ND A Ag Na A.7 MO+ Mao, K K 『ーu G.54 O AGCI

Using this table of standard reduction potentials determine which of the following is the strongest reducing agent. Hall Reon Nall 020 040 A+-A" 1.99 Aga+ Ag a 50++ S0, + RO 1.7N 0.22 C Ce PO Ot + S0 e AS, 20 189 M HO 1.51 As -Aa NO N LO a. 2 20 1.50 L4 Sa+- Se Nh N PARO, + S so -4.2) 1.3 13 .21 Ma + 4T M HO 10 4 • O LO9 Za Za LO0 Ma + Me NO NO + 280 -23 -237 -I7 -231 -2% -20 2 ND A Ag Na A.7 MO+ Mao, K K 『ーu G.54 O AGCI

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...

See similar textbooks

Similar questions

Consider the following redox reaction, and answer the three questions below.2MnO−4(aq)+2H2O(l)+6H+(aq) -----> 2Mn2+(aq)+5H2O2(l)The standard reduction potentials of the species in the reaction above are:H2O2(l)+2H+(aq)+2e− ----> 2H2O(l) E°red,H2O2 = 1.776 VMnO−4(aq)+8H+(aq)+5e−. ----> Mn2+(aq)+4H2O(l) E°red,MnO4- = 1.507 V Calculate E°. Calculate ΔG° Determine the equilibrium constant for the reaction.
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
Given the following electrochemical cell, calculate the potential for the cell in which the concentration of Ag+ is 0.0765 M, the pH of the H* cell is 2.700, and the pressure for H₂ is held constant at 1 atm. The temperature is held constant at 55°C. Ag Agt H+ + Ag+le ←H₂(g) Standard reduction potentials: 2H+ + 2e H₂ Fº = 0 V → Ag E°=0.800 V
Consider the reaction below:2 Ag(aq) + +Fe(s) → 2 Ag(s) + Fe^2+(aq) ΔG° = −241.0kJmol a. Calculate the equilibrium constant for this reaction.b. Calculate the standard cell potential for this reaction.
Identify the strongest reducing agent based on the following half- reactions. 2+ +1.22 V → Mn (aq) + 2H₂O(1) +0.61 V MnO₂(s) + 4H* (aq) + 2e- Hg₂SO4(s) + 2e → 2Hg(1) + SO4 (aq) SnO₂(s) + 2H₂O0+ 4e → Sn(s) + 4OH(aq) Cr(OH)3(s) + 3e → Cr(s) + 3OH(aq) -0.95 V -1.48 V Cr Mn02 Hg2SO4 Sn Hg
Given the following electrochemical cell, calculate the potential for the cell in which the concentration of Ag+ is 0.0765 M, the pH of the H* cell is 2.700, and the pressure for H₂ is held constant at 1 atm. The temperature is held constant at 55°C. Ag Ag+ H+ Standard reduction potentials: 2H+ +2e¯ → H₂ Eº = 0 V Ag+ le - H₂(g) → Ag Eº=0.800 V
D) AGO> 0 because AS Eº = +V A³+ (aq) + 3M(s) → 3 M* (aq) + A(s) 7. The redox reaction shown above is common in batteries and has a voltage equal to +V under standard conditions. Which of the following would occur if the standard 1 molar Mt solution was replaced with a 2 M solution? с altogo of the cell would increase as Q is greater than 1.