4. Build a voltaic cell with one beaker containing a solution of nickel (II) nitrate - Ni(NO3)2- with a nickel electrode, and a second beaker containing a solution of zinc chloride -ZnCl2 - with a zinc electrode.a. The half reactionsb. Flow of electronsc. Short-form notationd. Electric potential (voltage) 1.What is the difference between an oxidation number and a valence number?

Step 1: 4. a. In a voltaic cell, anode is the place where oxidation occurs, there is a loss of…

Answered: 4. Build a voltaic cell with one beaker…

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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The following are metal pairs representing electrodes in theoretical voltaic cells. Which pair is incorrectly labeled? a. Cu, reduced/ Pb, oxidized b. Ni, reduced/ Al, oxidized c. Na, oxidized/ Mg, reduced d. Ag, oxidized/Au, reduced O e. Ag, oxidized/ Cu, reduced
Suppose a battery is constructed with all of the concentrations of aqueous ions at 1M and the partial pressures at 1 atm. What is the voltage of this cell? A. Eº B. E cell C.0 cell
How many minutes will it take to plate out 4.56 g of Ni metal from a solution of Ni2+ using a current of 55.5 A in an electrolytic cell? A. 2.25 B. 270 C. 9.50 D. 135 E. 4.50
19. The following choices are primary batteries, along with their metal electrodes stated in parenthesis. Which of the following primary batteries will produce the most electrical energy if all the batteries stated are used for an hour? You can refer to the electrochemical series to determine the number of electrons produced by the metal substance. Assume all half-cell reactions are spontaneous. a. Aluminum-zinc battery b. Calcium-lead battery, c. Potassium-sodium battery d. Calcium-zinc battery
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?
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.
1.Ca metal is produced by electrolysis of __________. a.CaCl2 b.CaSO4 c.CaF2 d.CaCO3 2.Which hydroxide of group 1 metal is the LEAST soluble? a.KOH b.LiOH c.CsOH d.NaOH
78. A voltaic cell consists of a Pb/Pb2 half-cell and a Cu/Cu2" half- cell at 25 C. The initial concentrations of Pb and Cu are 0.0500 M and 1.50 M, respectively. a. What is the initial cell potential? b. What is the cell potential when the concentration of Cu2" has fallen to 0.200 M? c. What are the concentrations of Pb- and Cu" when the cell potential falls to 0.35 V?
4
The mostly familiar known .37 standard cell is Fuel cell .A B. Le Clanche C. Electrolytic cell D. Weston Cell O O A

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