4. For the following redox reaction in a galvanic cell, write the oxidation half-reaction and the reduction-half reaction, and calculate the standardcell potential of the reaction. Use Table 1 from the background as needed. Explain how you identified which substance was oxidized and which wasreduced. Show all of your work.Redox reaction: Cu(s) + 2 Fe* (aq) → Cu?+ (aq) + 2 Fe* (aq)Table 1. Standard reduction potentials.Half-ReactionE°(Volts)F,(g) + 2e → 2F (aq)CI, (g) + 2e → 2CI(aq)Br, () + 2e → 2Br(aq)Ag*(aq) + e¯ → Ag(s)+2.87+1.36+1.07+0.80Fe*(aq) + e → Fe²"(aq)+0.77Cu²*(aq) + 2e' → Cu(s)+0.342H*(aq) + 2e¯ → H,(g)0.00Fe2*(aq) + 2e' → Fe(s)-0.44Zn*(aq) + 2e' → Zn(s)-0.76Al³*(aq) + 3e' → Al(s)-1.66Mg"(aq) + 2e' → Mg(s)-2.37Ca²"(aq) + 2e" → Ca(s)-2.87K*(aq) + e' → K(s)-2.93ВUTTO Word(s)

Oxidation In which element loose electron and reduction in which element gain electron

4. For the following redox reaction in a galvanic cell, write the oxidation half-reaction and the reduction-half read cell potential of the reaction. Use Table 1 from the background as needed. Explain how you identified which subs reduced. Show all of your work. Redox reaction: Cu(s) + 2 Fe** (aq) –→ Cu²+ (aq) + 2 Fe²" (aq) Table 1. Standard reduction potentials. Half-Reaction E°(Volts) F,(g) + 2e → 2F(aq) CI,(g) + 2e → 2CI(aq) Br, () + 2e → 2Br(aq) Ag*(aq) + e¨ → Ag(s) Fe (aq) + e¯ → Fe²"(aq) +2.87 +1.36 +1.07 +0.80 +0.77 Cu2"(aq) + 2e' → Cu(s) +0.34 2H*(aq) + 2e¨ → H,(g) Fe2*(aq) + 2e' → Fe(s) Zn²*(aq) + 2e' → Zn(s) 0.00 -0.44 -0.76 Al³*(aq) + 3e' → Al(s) -1.66 Mg2 (aq) + 2e' → Mg(s) Ca2 (aq) + 2e' → Ca(s) -2.37 -2.87 K*(aq) + e' → K(s) -2.93 BIU = E T T;

4. For the following redox reaction in a galvanic cell, write the oxidation half-reaction and the reduction-half read cell potential of the reaction. Use Table 1 from the background as needed. Explain how you identified which subs reduced. Show all of your work. Redox reaction: Cu(s) + 2 Fe** (aq) –→ Cu²+ (aq) + 2 Fe²" (aq) Table 1. Standard reduction potentials. Half-Reaction E°(Volts) F,(g) + 2e → 2F(aq) CI,(g) + 2e → 2CI(aq) Br, () + 2e → 2Br(aq) Ag(aq) + e¨ → Ag(s) Fe (aq) + e¯ → Fe²"(aq) +2.87 +1.36 +1.07 +0.80 +0.77 Cu2"(aq) + 2e' → Cu(s) +0.34 2H(aq) + 2e¨ → H,(g) Fe2(aq) + 2e' → Fe(s) Zn²(aq) + 2e' → Zn(s) 0.00 -0.44 -0.76 Al³(aq) + 3e' → Al(s) -1.66 Mg2 (aq) + 2e' → Mg(s) Ca2 (aq) + 2e' → Ca(s) -2.37 -2.87 K(aq) + e' → K(s) -2.93 BIU = E T T;

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

For the question below find the standard change in free energy and the equilibrium constant for the galvanic cell resulting from the cell notation provided below. Use the standard reduction potentials from Appendix Cu(s) + Sn2+(aq) = Sn(s) + Cu2+(aq)
The standard EMF for the cell using the overall cell reaction below is +0.65 V: 2AI (s) + 312 (s) What is AGO for the cell reaction in kJ? Express your answer in decimal notation to one decimal place, without units. 2A1³+ (aq) + 61¯ (aq) →>>
Calculate the cell potential for the reaction as written at 25.00 degrees * C , given that [Zn^ 2+ ]=0.81 and [Sn^ 2+ ]=0.0190M M. Use the standard reduction potentials in this table. Zn(s)+ Sn ^ 2+ (aq) rightleftharpoons Zn^ 2+ (aq)+Sn(s)
A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Br2(1) + Mn(s) 2Br"(aq) + Mn2+(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: Enter the reaction that takes place at the cathode. Include state symbols: In the external circuit, electrons migrate the Mn electrode the Br2 electrode. Anions migrate the salt bridge the Br2 compartment.
Consider a voltaic cell in which the reaction is Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g) It is found that the cell voltage is +0.530 V when [Zn2+] = 1.0 M, PH2 = 1.0 atm. What must be the concentration of H+ in the cell? (Use the following information) (Show your work) 2H+ (aq) + 2e- → H2 (g) Eºred = 0.000 V Zn2+ (aq) + 2e- → Zn(s) Eºred = -0.762 V
write the answers properly
Which of the following is the correct shorthand notation for the overall cell reaction given below. Mg(s) + Cu2+(aq) → Mg2+(aq) + Cu(s) Select one: a. Mg(s) | Mg2+(aq) || Cu2+(aq) | Cu(s) b. Cu(s) | Mg2+(aq) || Cu2+(aq) | Mg(s) c. Mg(s) | Cu2+(aq) || Mg2+(aq) | Cu(s) d. Cu(s) | Cu2+(aq) || Mg2+(aq) | Mg(s)
What will be the products of the electrolysis of an 1-M aqueous aluminum chloride (AICI3) solution at 25 °C? (The electrodes themselves are platinum.) (Use the standard electrode potentials table in your online textbook's Appendix to help you answer the question.) No products will be produced. H₂(8) +20H (aq) + Cl₂(g) 4Al(s) + 30₂(g) + 12H*(aq) O 2H₂(g) + 4H₂O(l) + O₂(g) O2Al(s) + 3Cl2(g)
Consider the cell diagram: Pb(s)|Pb(NO3)2(aq)||FeCl3(aq)|Fe(s). Write the balanced net-ionic equations for the half-reactions that occur at the two electrodes. a. Anode= b. Cathode=
In each , decide whether the property measured was a chemical or physical property of X, if you can. If you don't have enough information to decide, choose can't decide in the third column. property R V H experiment Into one chamber of an electrochemical cell, a solution of X is introduced, along with a metal electrode. In the other chamber a solution of a known oxidizing reagent O is introduced, along with another metal electrode. The voltage across the electrodes is proportional to the tendency of O to react with X. By measuring this voltage, the value of R may be calculated. A sample of X is melted and put into a reservoir from which a very thin tube leads down. The rate at which X flows out of the tube is measured, and from this rate the value of V may be calculated. A sample of X is carefully weighed and put inside a sealed calorimeter. The calorimeter is heated electrically, and the amount of heat added determined by monitoring the electrical current used. The temperature of X is…
Consider the following half reactions: M²+ (aq) + 2e (aq) → M(S) X³+ (aq) + 3e (aq) →→→→→→X(s) Eº=-0.4 Eº=-0.7 Calculate the overall cell potential for the overall spontaneous redox reaction. Give your answer to one decimal place.
The redox reaction below has a ΔG° value of 315. kJ. Determine the standard cell potential(E°cell) for this reaction. A2+(aq) + 2B2+(aq) → A4+(aq) + 2B+(aq) Given the reaction below, complete the line notation. Co(s) + Cu2+(aq) → Cu+(aq) + Co2+(aq)