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: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 160MP

See similar textbooks

Similar questions

The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)
At 298 K, the solubility product constant for solid Ba(IO3)2 is 1.5 109. Use the standard reduction potential of Ba2+(aq) to find the standard potential for the half-reaction Ba(IO3)2(s)+2eBa(s)+2IO3(aq)
a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).
At 298 K, the solubility product constant for Pb(IO3)2 is 2.6 1013, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction Pb(IO3)2(s)+2ePb(s)+2IO3(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions, and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/Pb(IO3)2 electrode in a 3.5 103 M solution of NaIO3.
At 298 K, the solubility product constant for PbC2O4 is 8.5 1010, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction PbC2O4(s)+2ePb(s)+C2O42(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/PbC2O4 electrode in a 0.025 M solution of Na2C2O4.
For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)
The standard potential of the cell reaction Ag+(aq)+Eu2+(aq)Ag(s)+Eu3+(aq) is E = +1.23 V. Use the tabulated standard potential of the silver half-reaction to find the standard reduction potential for the europium half-reaction.
A half-cell that consists of a copper wire in a 1.00 M Cu(NO3)2 solution is connected by a salt bridge to a solution that is 1.00 M in both Pu3+ and Pu4+, and contains an inert metal electrode. The voltage of the cell is 0.642 V, with the copper as the negative electrode. (a) Write the half-reactions and the overall equation for the spontaneous chemical reaction. (b) Use the standard potential of the copper half-reaction, with the voltage of the cell, to calculate the standard reduction potential for the plutonium half-reaction.