4. At which electrode in a voltaic cell does reduction always occur?5. The diagram below is of a voltaic cell with magnesium and aluminum.A. Label the anode and cathode as either Al or Mg.UB. Using arrows indicate the flow of electrons.C. Using your reduction potential table, write the half reactions thatalong occur for oxidation and reduction in the spaces underneath thethe ax drawing.action Also, use the copperD. Using the values from the reduction potential table, calculate thevoltage of the cell.NOORMCONM.Total Ecell2018 ST←OT+01bosibisWrite the half-reactions that occur when a solid piece of silver is dipped into a solution of lithium nitrate.Half Reaction for Agof the cell?E Ag00+0 0 +18ELi and the cathede. Indicate theHalf Reaction for Lige and wire to complete the diagram below. LabelCincton the electrons would flow in the ware with ant

Note: As per the guidelines, solution of 4th and 5th question has been made. For the expert solution…

4. At which electrode in a voltaic cell does reduction always occur? 5. The diagram below is of a voltaic cell with magnesium and aluminum. A. Label the anode and cathode as either Al or Mg. B. Using arrows indicate the flow of electrons. C. Using your reduction potential table, write the half reactions that along occur for oxidation and reduction in the spaces underneath the the ax drawing. eaction Also, ase the copper a gaio D. Using the values from the reduction potential table, calculate the voltage of the cell. ORM 2018 ST bosibi

4. At which electrode in a voltaic cell does reduction always occur? 5. The diagram below is of a voltaic cell with magnesium and aluminum. A. Label the anode and cathode as either Al or Mg. B. Using arrows indicate the flow of electrons. C. Using your reduction potential table, write the half reactions that along occur for oxidation and reduction in the spaces underneath the the ax drawing. eaction Also, ase the copper a gaio D. Using the values from the reduction potential table, calculate the voltage of the cell. ORM 2018 ST bosibi

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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Use the standard reduction potentials in the table to create a galvanic cell with the highest possible standard cell voltage. Half-Reaction E°(Volts) F,(g) + 2e → 2F(aq) CI,(g) + 2e¯ → 2CI{aq) Br, (1) + 2e → 2Br(aq) +2.87 +1.36 +1.07 Agʻ(aq) + e' → Ag(s) +0.80 Fe (aq) + e → Fe²"(aq) +0.77 Cu2(aq) + 2e → Cu(s) 2H*(aq) + 2e¯ → H,(g) Fe2*(aq) + 2e →> Fe(s) Zn²*(aq) + 2e" → Zn(s) +0.34 0.00 -0.44 -0.76 Al³*(aq) + 3e' → Al(s) -1.66 Mg2 (aq) + 2e → Mg(s) -2.37 Ca2 (aq) + 2e¯ → Ca(s) -2.87 K*(aq) + e → K(s) -2.93
A common shorthand way to represent a voltaic cell is anode& anode solution& & cathode solution&cathode A double vertical line represents a salt bridge or a porous barrier. A single vertical line represents a change in phase, such as from solid to solution. Using the notation just described, represent a cell based on the following reaction: ClO3 -1aq2 + 3 Cu1s2 + 6 H+1aq2 ¡ Cl -1aq2 + 3 Cu2+1aq2 + 3 H2O1l2 Pt is used as an inert electrode in contact with the ClO3 - and Cl -. Calculate the standard cell emf given: ClO3 -1aq2 + 6 H+1aq2 + 6 e- ¡ Cl -1aq2 + 3 H2O1l2; E° = 1.45 V.
A student measures the voltage across different metal electrodes placed in a voltaic cell. Using a tin cathode, the voltages when using a first an aluminum, then copper anode are positive and negative, respectively. The order of chemical reactivity of the solid metals must be a.Cu>Sn>Al b.Al=Cu>Sn c. Al=Cu d.Al>Sn>Cu
1. Use the standard reduction potentials in the table to create a galvanic cell with the highest possible standard cell voltage. 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)
The technique of protecting a metal from corrosion by connecting it to a second metal that is more easily oxidized is called cathodic protection. Which of the following metals would be suitable for the cathodic protection of iron? Refer to the standard reduction potential table. A. Al B. Cu C. Ag D. Ni
Which of the following statements is(are) true for all galvanic cells? 1. Reduction occurs at the cathode. II. The anode gains mass during discharge (note: this means operation of the cell.) III. The voltage is less than or equal to zero. O only I O only III O only II O L I, and II O Il and II
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.
Write the oxidation half-reaction and reduction half-reaction, and shorthand electrochemical notation for the following. Even without a solution. Thank you ?! D. 3 Hg2+ + 2 Fe(s) -> 3 Hg2 + 2 Fe3+ E. 2As(s) + 3Cl2 (g) -> 2AsCl3 F.
24. What will happen if a student measures the voltage of a voltaic cell where the student mixed the two half-cells together without separating them with a salt bridge? The student will probably experience an electrical shock. The reaction will happen much more rapidly so register a higher voltage. No reaction will occur without a salt bridge. No voltage will be recorded.
Which one of the following statements is true? Select all that apply. A. B. 5 poin An electrolytic cell does not require external voltage to operate. Reduction occurs at the cathode in a galvanic cell. C.Oxidation occurs at the anode in a galvanic cell but not in an electrolytic cell. D.Oxidation occurs at the cathode in an electrolytic cell. E. When a galvanic cell is recharged, the reverse chemical reaction occurs as when the galvanic cell operates.