Use the standard reductionpotentials in the table to create agalvanic cell with the highest possiblestandard cell voltage.Half-ReactionE°(Volts)F,(g) + 2e → 2F(aq)CI,(g) + 2e¯ → 2CI{aq)Br, (1) + 2e → 2Br(aq)+2.87+1.36+1.07Agʻ(aq) + e' → Ag(s)+0.80Fe (aq) + e → Fe²"(aq)+0.77Cu2(aq) + 2e → Cu(s)2H*(aq) + 2e¯ → H,(g)Fe2*(aq) + 2e →> Fe(s)Zn²*(aq) + 2e" → Zn(s)+0.340.00-0.44-0.76Al³*(aq) + 3e' → Al(s)-1.66Mg2 (aq) + 2e → Mg(s)-2.37Ca2 (aq) + 2e¯ → Ca(s)-2.87K*(aq) + e → K(s)-2.93 a. Write the oxidation half-reaction.b. Write the reduction half-reaction.c. Calculate the standard cellvoltage.d. Write the overall cell reaction(redox reaction)

We will find anode and cathode and then find cell pot and reaction.

Answered: a. Write the oxidation half- reaction.…

a. Write the oxidation half- reaction. b. Write the reduction half- reaction. c. Calculate the standard cell voltage. d. Write the overall cell reaction (redox reaction)

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

8. Out of the following statements, which is incorrect? In a galvanic cell: a. The oxidation takes place at the anode. b. The reduction takes place at the cathode. C. The positive electrode is located at the cathode. d. The negative electrode is located at the cathode. Electrons travel in the wire from anode to cathode. e.
An iron electrode in a solution of iron (II) nitrate and a magnesium strip in a solution of magnesium nitrate form a galvanic cell. The size of the magnesium strip is observed to decrease over time. Sodium nitrate is found in the salt bridge. a, Sketch a diagram of the cell. Include all substances on the diagram. b, Label the anode and the cathode. c, Write out the two half-reactions and the overall cell reaction. d, On the diagram Indicate the direction of electron flow, the direction the reactants are moving, and the direction the ions in the salt bridge are moving.
6. Consider a galvanic cell consisting of an Al electrode placed in a 1 M Al(NO3)3 solution and a Ag electrode placed in a 1 M AgNO3 solution. a.)Write the half-reaction which occurs at the anode. b.)Write the half-reaction which occurs at the cathode c.)Write a balanced net ionic equation for the galvanic cell. d.)Calculate the standard emf of the cell e.)Give the cell diagram for the reaction occurring in this galvanic cell. f.)What is oxidized? g.)What is the oxidizing agent?
The Nernst equation can be used to calculate... A. cell potentials from standard cell potentials when the conditions of concentration and temperature are not standard B. standard cell potentials from standard reduction potentials C. cell potentials given only the temperature and reactant concentrations D. cell potentials from standard oxidation potentials E. the change in standard Gibbs free energy from standard cell potentials
C(13) Please help me answer this one! I need an urgent answer for this. | Consider a cell containing NaCl. a. Draw a diagram of a cell for electrolysis of molten NaCl. Label the anode and cathode. b. Write the equations for the anode and cathode half-reactions and the overall reaction.
1.Represent in the conventional manner, i.e., anode/cathode, the voltaic cell in which each of the following reactions occur spontaneously. A. Zn + Ni2* → Zn2* + Ni B. 2AI + 3CI2 → 2AICI3 С. Н2 + 2Ag* → 2H* +2Ag D. 2H* + Pb → H2 Pb2+ + 2. Write the half reactions occurring at the cathode and at the anode when each cell shown in problem #1 is delivering current. 3. Calculate the voltage of the cell shown in problem #1.
O ELECTROCHEMISTRY Designing a galvanic cell from two half-reactions A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential half-reaction 2+ Fe (aq) Ed=+0.771 V %3D 3+ red Fe"(aq)+e Cro (aq)+4 H,O(1)+3e Cr(OH),(s)+5OH (aq) -0.13 V Ered nswer the following questions about this cell. Jrite a balanced quation for the alf-reaction that appens at the athode. rite a balanced uation for the If-reaction that ppens at the ode. ite a balanced uation for the erall reaction
Danial cell is an example of .A Concentration cell .B Galvanic cell .C Electrolytic cell .D none
1) How are the terms “electrochemical cell” and “battery” related? 2) Give a brief description of how and why a battery works. 3) There are two types of batteries: Primary and secondary. How are these types of batteries different from one another? How are they the same?
B. Redox reaction 24. Which of the following refers to a hypothetical reaction that shows only the oxidation or reduction reaction? A. Addition Reaction C. Endothermic reaction 25. What part of the electrochemical cell allows ions to flow back and forth so that charge does not build up? B. Cathode C. Motor A. Anode D. Half-reaction D. Salt bridge
An electrochemical cell has a positive standard cell potential but a negative cell potential. Which statement is true? a. K> 1; Q > K b. K K c. K> 1; Q < K d. K< 1; Q< K
1) Construct a zinc-copper electrochemical cell using 1.0 M Zn2+ and 1.0 M Ni2+ solutions. a. Provide the shorthand notation. b. What is the EMF of this cell (include units)? c. For the voltage that you are measuring, is this E°cell or Ecell? Explain.