Answer the questions for the cell diagram shown below.I H₂ (g)Ni(s) Ni+22H(aq)(aq)12. Write the half reaction that is happening at theanode.13. Write the half reaction that is happening at thecathode.Fl. Calculate the Ę for this reaction.15. What type of cell must this redox reaction beoccuring in?Cd(aq) +le-Cd(s) SRP -0.40 VAu +1 e-(aq)2 W av + 2e-H₂> SRP == -0.257 V-)

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Answered: Answer the questions for the cell…

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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An electrochemical cell uses Ag and Zn as electrodes. Based on the reduction potentials, the (blank) electrode is where the reduction will occur and it is called the (blank) a.Ag, cathode b.Zn, anode c.Ag, anode Based on the reactions below, which is the stongest reducing agent? +1.22 V MnO2(s) + 4H+(aq) + 2e- → Mn2+(aq) + 2H2O(1) +0.61 V Hg2SO4(s) + 2e- → 2Hg(1) + SO4 2- (aq) -0.95 V SnO2(s) + 2H2O() + 4e-→ Sn(s) + 40H-(aq) -1.48 V Cr(OH)3(s) + 3e- → Cr(s) + 3OH-(aq) a.Hg2SO4 b.Mn02 c.Cr d.Sn e.Hg Identify the strongest oxidizing agent from the following half-reactions. The standard reduction potentials are listed. +1.22 V Mn02(s) + 4H+(aq) + 2e- → Mn2+(aq) + 2H20(1) +0.61 V Hg2SO4(s) + 2e- → 2Hg(1) + SO4 2-(aq) -0.95 V SnO2 (s) + 2H2O() + 4e- Sn(s) + 40H-(aq) -1.48 V Cr(OH)3(s) + 3e- Cr(s) + 3OH- (aq) a. MnO2 b.Hg2SO4 c.Sn d.Hg e.Cr
For the electrochemical cell represented by this shorthand notation, which statement below is true? Ni | Ni2+ || Ti3+, Ti2+ | Pt Ti3+ + e– → Ti2+ E° = –0.37 V Ni2+ + 2e– → Ni E° = –0.257 A. Platinum is the cathode and is positive B. Nickel is the cathode and is positive C. Platinum is the cathode and is negative D. Nickel is the cathode and is negative
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2 H₂O(1)+2e →> H2(g)+2 OH (aq) E.ed = -0.83 V red Cu²+(aq)+e Cu+ (aq) →>> Answer the following questions about this cell. E° = +0.153 V red Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the ☐ ☐
A cell utilizes the following reaction and operates at 298 K: 2H+(aq) + Zn(s) → Zn2+(aq) + H2(g) a.What is the emf of this cell under standard conditions? (Look up E° values). b. What is the emf of this cell when [Zn2+] = 0.050 M, PH2 = 0.25 atm, and the pH = 4.00.(Use pH toget [H+]
For each of the electrolyte electrode pairings, indicate the oxidation reaction, the reduction reaction, the cell reaction, and the overall expected EMF of the cell using the tables. Write the conventional cell notation. a. Zn and Zn² mixed with Pb and Pb+² b. Cu and Cu2 mixed with Ag and Ag*
11. The following two half-cells are connected to form a full Galvanic cell: Cu"(aq) +2e Au (aq) +e → Cu(s) → Au(s) E° = 0.34 V E 1.69 V a. Calculate E° for the cell. b. Give the cell notation for this system. c. Give the balanced cell reaction. d. Calculate AG for the reaction e. Calculate Keg for the reaction. £. Calculate the cell potential if the activity of Cu is 0.0100 and the activity of Au" is 1.340.
need help with this chemistry
signs a galvanic cell that uses these two half-reactions: half-reaction 2 H₂O(1)+2e H₂(g) + 2OH(aq) 3+ 2+ Fe³+ (aq)+e → Fe²+ (aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. A chem standard reduction potential E-0.83 V red E 'red = +0.771 V 2H₂O(1) + 2e → H₂(g) + 2OH(aq) 2+ 3+ Fe → Fe (aq) + e 7 ロ→ロ e X x10 Ś ?

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