Suppose the following reaction happening at 25°CSn(s) + CuSO4(aq)SNSO4(aq) (reaction in equilibrium)Cu(s) +<-----a) Write the left (Anode) and right (Cathode)reactions.b) Calculate the standard cell potential E°Cell·c) Calculate the equilibrium constant “K" of thereaction using the standard potential data table.TABLE 17.1 Standard Reduction Potentials at 25°C (298 K) for Many Common Half-ReactionsHalf-Reactione (V)Half-Reactione° (V)F + 2e 2FAg* +e - Ag"Co +e →CơH,O, + 2H + 2e 2H,0Ce +e → Ce*PbO, + 4H + so + 2e PbSO, + 2H,0MnO, + 4H* + 3e MnO, + 2H,O2e + 2H + IO, 10, + H,0MnO, + 8H + Se" → Mn* + 4H,0Au + 3e -→ AuPbO, + 4H + 2e Pb* + 2H,OCa, + 2e" → 2CI"Cr0,- + 14H + 6e" → 2Cr“ + 7H,0O, + 4H + 4e 2H,OMnO, + 4H + 2e Mn + 2H,O10, + 6H + Se → I, + 3H,0Br, + 2e 2Br-2H +e VO + H,O2.871.99O, + 2H,0 + 4c → 40HCu + 2e CuHg,Cl, + 2e -→ 2Hg + 2CIAgCI +e Ag + CIso- + 4H + 2e → H,SO, + H,OCu* + e - Cu*2H + 2e H;Fe + 3e FePb* + 2e" -→ PbSnNi* + 2e NiPbSO, + 2e - Pb + So,-Cd + 2e -→ CdFe* + 2e FeCr* +e Cr*Cr + 3e → CrZn* + 2e - Zn0.400.341.820.271.780.221.700.201.691.680.160,001.60-0.0361.51-0.132e Sn1.501.461.36-0.14-0.23-0.35-0.401.331.23-0,441.21-0,501.20-0.731.09-0.76-0.83VO,AuCl, + 3e → Au + 4CINO, + 4H + 3e NO + 2H,OCIO, +e → CIO,2Hg* + 2e Hg,*Ag +e → AgHg, + 2e 2HgFe +e → Fe*O, + 2H* + 2e" → H;O;MnO, +e -→ MnO,I, + 2e 21Cu +e Cu1.002H,0 + 2e - H, + 20HMn + 2e"- MnAl + 3e → AlH + 2e 2HMg + 2e MgLa + 3e -→ LaNa + e → NaCa + 2e -→ CaBa + 2e" - Ba-1.18-1.660.990.960.954-2.23-2.37-2.37-2.71-2.760.910,800.800.770.68-2.900.56K* +e - K-2.920.54Li +e Li-3.050.52

In an electrochemical cell, the electrical energy is produced from the spontaneous cell reaction at…

Suppose the following reaction happening at 25°C Sn(s) + CuSO4(aq) <-----¯ Cu(s) + SNSO4(aq) (reaction in equilibrium) a) Write the left (Anode) and right (Cathode) reactions. b) Calculate the standard cell potential E°Cell- c) Calculate the equilibrium constant “K" of the reaction using the standard potential data table.

Suppose the following reaction happening at 25°C Sn(s) + CuSO4(aq) <-----¯ Cu(s) + SNSO4(aq) (reaction in equilibrium) a) Write the left (Anode) and right (Cathode) reactions. b) Calculate the standard cell potential E°Cell- c) Calculate the equilibrium constant “K" of the reaction using the standard potential data table.

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

1 2 B A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown: Co2(aq) + 2e Co(s) E° -0.28 volt; Cd2+ (aq) + 2e-Cd(s) E°--0.42 volt. What is the standard free energy change in kJ for the cell reaction of this galvanic cell? Report your answer in whole number. Do not put unit in your answer. Type your answer...
Kindly write the sol.n
Part A If a voltaic cell is created between a Am"/Am electrode and a Fe*/Fe electrode, what species is being oxidized? O Am"(ag) O Fe(s) O Fe"(ag) O Am(s)
The potential of the following voltaic cell is 0.55 V. Given this information, determinethe Kb for the organic base (RNH2) dissolved in the left cell.
MnO4– + Sn ----> MnO2 + Sn2+ A) Identify the half-reaction that occurs at the cathode. B) Identify the oxidizing agent and anode. C) standard cell potential? D) What will be the potential of a cell constructed using 57.0 g MnO2, 1.57 M MnO4–, 14.8 g Pt, 12.5 g Sn and 0.87 M Sn2+ at pH 2.5?
Will the cell reaction proceed spontaneously as written for the following cell? Sn (s) | Sn2+ (0.50 M) || Pb2+ (0.0010 M) | Pb (s) b) What is the value of for the cell reaction?
Consider the following half-reactions: Half-reaction E° (V) Cl2(g) + 2e" → 2CI'(aq) 1.360v Ni?*(aq) + 2e- Ni(s) |-0.250V 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 Cl'(aq) to Cl2(g)? (6) Which species can be reduced by Ni(s)? If none, leave box blank.
Referring to the table of Standard Cell Potentials below, determine the standard cell potential for the following reaction: Pb2+(aq) + 2 Cl-(aq) ---> Pb(s) + Cl2 E° Pb2+(aq) + 2e- ---> Pb(s) -0.126 Cl2 + 2e- ---> 2 Cl-(aq) +1.360
Calculate values for the galvanic cells described below. (a) Cr³+ (aq) + Cl₂(g) Cr₂O7²-¯(aq) + Cl¯ (aq) (b) Zn(s) + Ag¹(aq) Zn²+ (aq) + Ag(s)
3) Draw a picture of the galvanic cell represented by the line notation below and then write the reduction half-reactions for each electrode. Also identify the anode and cathode for each half cell. Pt (s) | Fe3+ (aq), Fe2+ (aq) || Cr2O72-(aq), Cr3+ (aq), HA (aq) | Pt (s)
An electrochemical cell consists of a silver metal electrode immersed in a solution with Ag* = 1.0 M separated by a porous disk from a copper metal electrode. If the copper electrode is placed in a solution of 5.0 MNH3 that is also 0.0080M in Cu(NH3),+, what is the cell potential at 25°C? Cu?+ (ag) + 4 NH3 (aq) = Cu(NH3)4²* (aq) K = 1.0 × 1013 Cell potential V
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