GENERAL INSTRUCTIONS Read and analyze carefully each problem. Solve for the standard cell potential and interpret the result. Make sure to identify the anode half-cell and the cathode half-cell, balance the half reactions, and write the over-all reaction. Show your complete solution. a. Ni2/Ni and Ag /Ag half-reactions b. Ca²/Ca and Cu2/Cu half-reactions c. Pb²+ + Au- • Au + Pb d. Ni+ Cu²N²2² + Cu e. Mn2+ SO4 SO₂ + MnO₂

GENERAL INSTRUCTIONS Read and analyze carefully each problem. Solve for the standard cell potential and interpret the result. Make sure to identify the anode half-cell and the cathode half-cell, balance the half reactions, and write the over-all reaction. Show your complete solution. a. Ni2/Ni and Ag /Ag half-reactions b. Ca²/Ca and Cu2/Cu half-reactions c. Pb²+ + Au- • Au + Pb d. Ni+ Cu²N²2² + Cu e. Mn2+ SO4 SO₂ + MnO₂

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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I need to determine the reduction potentials of all other half-lifes using reduction potential of Zn^2+ (0.10)/Zn half-reaction. I included the data for one of the half-lives I need to find. The known reduction potential for Zn^2+/Zn is -0.79 The cathode is Cu and the anode is Fe The potential (V) for this half cell is 0.767 and it is the potential for the Ecell. The concentration of Cu(NO3)2 is 0.10M and the concentration of Fe(NO)3 is 0.10M In the Cu/Zn pairing the supposed reduction potential of Cu was 0.212. The instructions said to use this value to determine reduction potential of Fe
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction MnO4(aq) + 2 H2O(l)+3e MnO2(s)+4OH(aq) Br₂(1)+2e →>> 2 Br (aq) standard reduction potential E = +0.59 V 'red E = +1.065 V 'red Answer the following questions about this cell.
A voltaic cell is set up with a Ni2+ (aq) /Ni (s) redox conjugate pair at the cathode. Select each redox conjugate pair that can be placed at the anode that will allow for spontaneous electron transfer: Mn²+/Mn Ba²+/Ba Pb²+/Pb H+/H₂ F₂/F²
Enter electrons as e. Use smallest possible integer coefficients. If a box is not needed, leave it blank. A voltaic electrochemical cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. 3Mn(s) + 2Cr³+(aq) - 3Mn²+ (aq) + 2Cr(s) What is the reaction that takes place in the anode compartment? + What is the reaction that takes place in the cathode compartment? + In the external circuit, electrons migrate electrode ✓the Cr3+ electrode. In the salt bridge, anions migrate compartment + the Cr³+ compartment. + the Mn the Mn
Consider a galvanic cell based in the reaction Fe2+ + Cr,O,→ Fe³+ + Cr³* . Cr,03- + 14H* + 6e¯ →2Cr+ + 7H,0 1.33 Fe+ + e→ Fe?+ 0.77 Balance the reaction. What is the coefficient of Fe3+ in the balanced equation? а. 3 b. 6 с. 4 d. 2 e. none of these
Part B – Measuring Electrode Potentials From your results, arrange these reductions in order of decreasing reduction potential: Get a sample tube and a piece of metal for each of the half-cells listed on the right. Also get one pre-assembled copper half-cell (as shown in the photo on the left below). 1. Half-Cells Zn²*(aq) + 2e Pb2+(aq) + 2e Zn(s) Zn2+ | Zn 2e Pb(s) Sn2+(aq) + Cu2*(aq) + 2. Half fill each sample tube with the 1 M solution of the appropriate metal cation. Sn(s) Pb2+ | Pb Sn2+ | Sn 2e Cu(s) 3. Insert a two holed plastic cap into each tube and insert the piece of clean metal (Zn, Pb, or Sn) appropriate to the cell into one hole. Each group should have a set of cells as pictured on the right below, Highest (most positive) reduction potential Pb Sn Lowest (least positive) reduction potential b2 /pb Sn2/ Zn2* 4. Starting with the Zn2+ | Zn half-cell, insert the copper half-cell into the second hole in the plastic cap (as shown in the picture below). Make sure the bottom of…
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Pb and Pb+2 mixed with Cd and Cd+2 a. determine the oxidation reaction b. determine the reduction reaction c. determine the cell reaction d. determine the expected EMF for the cell
What is the standard emf of the cell with the following overall reaction? Use the provided table for the standard reduction potentials of half-reactions. 2Fe2+ + 2Hg2+2Fe3+ + Hg22+ Express your answer in two decimal places. Table 11.1 Standard Reduction Potentials at 25°C (298 K) for Many Common Half-reactions Half-reaction F₂+2e-2F- Ag²+ + e → Ag' Co" te - Cot H₂O₂ + 2H+ + 2e →> Ce+eCe³+ PbO₂ + 4H+ SO4 MnO4 + 4H+ 3e 10₁ + 2H+ 2e MnO4 + 8H + Se Au +3e Au PbO₂ + 4H¹ + 2e → Pb²+ + 2H₂O Cl₂ + 2e → 2CI Cr₂O₂ + 14H+6e2Cr³+ + 7H₂O 2H₂0 +2e → PbSO4 + 2H₂O MnO₂ + 2H₂O 10, + H₂O O₂ + 4H+ 4e → 2H₂O MnO₂ + 4H+ 2e →Mn² + 2H₂O 12+ 3H₂O 10, + 6H + Se Br₂ +2e7 →2Br VO₂ + 2H+ c→ VO²+ + H₂O AuCl +3e7 → Au + 4CI™ NO3 + 4H+ 3e7 CIO₂+eClO₂ 2Hg2+2e7 → Hg₂+ Ag +eAg Hg₂+2e → 2Hg Fe³+ + c →Fe²+ Cu Mn² + 4H₂O → NO + 2H₂O O₂ + 2H+ 2e H₂O₂ MnO4 + MnO2- 12+ 2e21 Cute 8° (V) 2.87 1.99 1.82 1.78 1.70 1.69 1.68 1.60 1.51 1.50 1.46 1.36 1.33 1.23 1.21 1.20 1.09 1.00 0.99 0.96 0.954 0.91 0.80 0.80 0.77 0.68 0.56 0.54…
A voltaic cell is constructed with a Cr/Cr3+ half-cell (E° = -0.73 V) and a Ni/Ni2+ half-cell (E° = -0.23 V).a. Write balanced half-reactions and the overall spontaneous reaction.b. Diagram the cell. Be a specific as possible including labeling electrodes with their charges and names (anode and cathode), showing the direction of electron flow in the circuit and showing the direction of cation and anion flow in the salt bridge.
Do not have to answer any questions. JUST WRITE THE OBJECTIVES IN YOUR OWN RODS: Objective: To measure Ecel for several voltaic cells and determine the standard potential for each half cell. To determine Ksp of AgCl and the K of [Cu(NH3)4]*.