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6. The following questions concern a battery based on the Cd2+/Cd (Cd = cadmium) and the Ag1+/Ag (Ag = silver) half-cells. NaCl(aq) is used in the salt bridge. The rele- Cl2(8) + 2 e 2 Cl1-(aq) +1.36 V %3D Pt2+(aq) + 2 e Pt(s) +1.18 V %3D HNO3(aq) + 3 H1+(aq) + 3 e NO(8) + 2 H2O(1) +0.96 V vant reactions and values of the Ag1+(aq) + 1e Ag(s) +0.80 V %3D standard reduction potentials are listed in the table at the right. Cu2+(aq) + 2 e Cu(s) +0.34 V %3D 2 HC(ад) + 2е H2(8) + 2 Cl1-(aq) 0.00 V %3D Cd2+(aq) + 2 e Cd(s) -0.40 V %3D Na1+(aq) + 1e Na(s) -2.71 V %3D Is each of the following statements true or false? Indicate your choice by circling T (if the statement is TRUE) or F (if the statement is FALSE). a. Electrons flow from the Cd2+/Cd half-cell to the Ag1+/Ag half-cell. T F b. The reducing agent is Ag(s) and the oxidizing agent is Cd2+(aq). T F С. The Agl+/Ag half-cell is the anode. T F

6. The following questions concern a battery based on the Cd2+/Cd (Cd = cadmium) and the Ag1+/Ag (Ag = silver) half-cells. NaCl(aq) is used in the salt bridge. The rele- Cl2(8) + 2 e 2 Cl1-(aq) +1.36 V %3D Pt2+(aq) + 2 e Pt(s) +1.18 V %3D HNO3(aq) + 3 H1+(aq) + 3 e NO(8) + 2 H2O(1) +0.96 V vant reactions and values of the Ag1+(aq) + 1e Ag(s) +0.80 V %3D standard reduction potentials are listed in the table at the right. Cu2+(aq) + 2 e Cu(s) +0.34 V %3D 2 HC(ад) + 2е H2(8) + 2 Cl1-(aq) 0.00 V %3D Cd2+(aq) + 2 e Cd(s) -0.40 V %3D Na1+(aq) + 1e Na(s) -2.71 V %3D Is each of the following statements true or false? Indicate your choice by circling T (if the statement is TRUE) or F (if the statement is FALSE). a. Electrons flow from the Cd2+/Cd half-cell to the Ag1+/Ag half-cell. T F b. The reducing agent is Ag(s) and the oxidizing agent is Cd2+(aq). T F С. The Agl+/Ag half-cell is the anode. T F

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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6. The following questions concern a battery based on the Cd²+/Cd (Cd = cadmium) and the Ag1+/Ag (Ag = silver) half-cells. NaCl(aq) is used in the salt bridge. The rele- Cl2(g) + 2 e 2 Cl1-(aq) +1.36 V Pt2+(aq) + 2 e Pt(s) +1.18 V HNO3(aq) + з н1+ (ад) + 3е NO(8) + 2 H2O(1) +0.96 V vant reactions and values of the Ag1+(aq) + 1e Ag(s) +0.80 V %3D standard reduction potentials are listed in the table at the right. Cu2+(aq) + 2 e Cu(s) +0.34 V 2 HCI(aд) + 2 е H2(g) + 2 Cl1-(aq) 0.00 V Cd2+(aq) + 2 e Cd(s) -0.40 V %3D Na1+(aq) + 1e Na(s) -2.71 V Is each of the following statements true or false? Indicate your choice by circling T (if the statement is TRUE) or F (if the statement is FALSE). Electrons flow from the Cd2+/Cd half-cell to the Ag1+/Ag half-cell. F а. b. The reducing agent is Ag(s) and the oxidizing agent is Cd2+(aq). T F C. The Ag1+/Ag half-cell is the anode. T F d. The Na1+(aq) ions move through the salt bridge toward the Ag1+/Ag half-cell. T F е. This battery will produce close to 0.40 volts of electrical energy. T F f. Na1+(aq) can be used instead of Ag1+(aq) in the Ag1+/Ag half-cell. F g. Ag(s) reacts with Pt2+(aq) but not with Cu2+(aq). T F h. Ag1+(aq) does not react with Pt(s). T F i. Nal+(aq) can be used instead of Cd(s) in the Cd2+/Cd half-cell. T F j. Ag(s) is a stronger reducing agent than Cu(s). T F k. Pt2+(aq) is a stronger oxidizing agent than HNO3(aq). T F 1. Sn, tin, is a more reactive metal than Ag. Substituting the Sn2+/Sn half-cell for the Ag1+/Ag half-cell will result in a battery that produces a larger voltage. F
Transcribed Image Text:6. The following questions concern a battery based on the Cd²+/Cd (Cd = cadmium) and the Ag1+/Ag (Ag = silver) half-cells. NaCl(aq) is used in the salt bridge. The rele- Cl2(g) + 2 e 2 Cl1-(aq) +1.36 V Pt2+(aq) + 2 e Pt(s) +1.18 V HNO3(aq) + з н1+ (ад) + 3е NO(8) + 2 H2O(1) +0.96 V vant reactions and values of the Ag1+(aq) + 1e Ag(s) +0.80 V %3D standard reduction potentials are listed in the table at the right. Cu2+(aq) + 2 e Cu(s) +0.34 V 2 HCI(aд) + 2 е H2(g) + 2 Cl1-(aq) 0.00 V Cd2+(aq) + 2 e Cd(s) -0.40 V %3D Na1+(aq) + 1e Na(s) -2.71 V Is each of the following statements true or false? Indicate your choice by circling T (if the statement is TRUE) or F (if the statement is FALSE). Electrons flow from the Cd2+/Cd half-cell to the Ag1+/Ag half-cell. F а. b. The reducing agent is Ag(s) and the oxidizing agent is Cd2+(aq). T F C. The Ag1+/Ag half-cell is the anode. T F d. The Na1+(aq) ions move through the salt bridge toward the Ag1+/Ag half-cell. T F е. This battery will produce close to 0.40 volts of electrical energy. T F f. Na1+(aq) can be used instead of Ag1+(aq) in the Ag1+/Ag half-cell. F g. Ag(s) reacts with Pt2+(aq) but not with Cu2+(aq). T F h. Ag1+(aq) does not react with Pt(s). T F i. Nal+(aq) can be used instead of Cd(s) in the Cd2+/Cd half-cell. T F j. Ag(s) is a stronger reducing agent than Cu(s). T F k. Pt2+(aq) is a stronger oxidizing agent than HNO3(aq). T F 1. Sn, tin, is a more reactive metal than Ag. Substituting the Sn2+/Sn half-cell for the Ag1+/Ag half-cell will result in a battery that produces a larger voltage. F
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