1. An electrochemical cell is made of two electrodes: (Zn²+/Zn) and (Ag*/Ag). Use the standard reductic potentials to answer the following questions. a. What is the standard potential of the cell and which electrode is the cathode and which one is the anode? b. Write a net redox equation for this electrochemical cell.

1. An electrochemical cell is made of two electrodes: (Zn²+/Zn) and (Ag*/Ag). Use the standard reductic potentials to answer the following questions. a. What is the standard potential of the cell and which electrode is the cathode and which one is the anode? b. Write a net redox equation for this electrochemical 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...

See similar textbooks

Similar questions

a. Given the following standard cell notation, draw and label the electrochemical cell. Be sure to label: anode, cathode, salt bridge, flow of electrons, flow of all ions. b. Write the half reactions for each half cell, and the net cell reaction. c. Calculate the cell potential. Mg(s) | Mg(NO3)2(aq) ||AgNO3(aq) [Ag(s)
A concentration cell is based on the aqueous reaction: Cu2+(1.00 M) ---> Cu2+(0.0100M) The cell consists of copper electrodes dipping into solutions of Cu2+ ions. The anions present are sulfate ions. Write the shorthand cell notation for this cell and draw the cell.
For the following voltaic cell:Fe(s) | Fe^2+(aq, 1.0 M) || Cu^2+(aq, 1.00 M) | Cu(s) a. Draw a diagram of the cell.b. Write the cell half-reactions.c. Label one half-reaction as the oxidation, the other as the reduction.
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?
74. A voltaic cell employs the redox reaction: Sn²+(aq) + Pb(s) Sn(s) + Pb2+(aq) E° cell = 0.010 V Calculate the cell potential, Ecell, at 25°C under each set of conditions. a. [Pb2+] = 0.010 M; [Sn²+] = 0.010 M b. [Pb2+] c. [Pb2+] = = 1.0 × 10 6 M; [Sn²+] = 2.0 M 1.5 M; [Sn2] = 0.010 M
1. What is the voltage for the reaction under standard conditions: 2Al(s) + 3Pb2+(aq) → 2Al3+(aq) + 3Pb(s)? 2.What is the voltage for the reaction under standard conditions: 3Ag(s) + Cr3+(aq) → 3Ag+(aq) +Cr(s)? (See above for reduction potentials.)
2.What is the standard cell potential of an electrochemical cell? A.the sum of standard electrode potential of the two half-cells B.the standard electrode potential of the anode, relative to a hydrogen cell C.the difference between the standard electrode potential of the two half-cells D.the standard electrode potential of the cathode, relative to a hydrogen cell
Calculate the cell potential for the reaction as written at 25.00 degrees * C , given that [Zn^ 2+ ]=0.81 and [Sn^ 2+ ]=0.0190M M. Use the standard reduction potentials in this table. Zn(s)+ Sn ^ 2+ (aq) rightleftharpoons Zn^ 2+ (aq)+Sn(s)
1a
2. The reduction of aluminum ions occurs as: Al³+ (aq) + 3e → Al(s) After applying a certain amount of current through an electrolytic cell, 0.1328 g of aluminum is deposited at the electrode a. How many moles of aluminum metal has been deposited? b.How many aluminum atoms have been deposited? (Use Avogadro's number). c. How many electrons were required for the reduction of this much aluminum? d. If the electronic charge is 1.60 x 10-¹C, what is the total electrical charge used? e. If a constant current of 90 mA were applied, what was the time elapsed in seconds and in minutes?
A cell is constructed by immersing a strip of silver in 0.10 M AgNO 3 solution and a strip of lead in 1.0 M Pb(NO 3) 2 solution. A wire and salt bridge complete the cell. What is the potential of the silver electrode in the cell? O a. 0.80 V O b. 0.83 V O C. 0.88 V O d. 0.86 V e. 0.74 V
Determine if the reaction below is spontaneous.Cl2(g) + 2 F–(aq) ⇌ F2(g) + 2 Cl–(aq)a. Based on the given reaction, write the reduction half-reaction.b. Based on the given reaction, write the oxidation half-reaction.c. By looking at the reduction potential table below, calculate the standard cell potential.