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n electrochemical cell is constructed in which both electrodes are pure iron immersed in a solution of Fe ions. The [Fe1] concentration for one half cell is 0.5 M and [Fe2] for the other half cell is 0.02 he temperature of the solution is 25 °C. Is a voltage generated between the two half-cells? If so, what is its magnitude and which electrode will be oxidized? NOTE: The symbol M is used to indicate "molar" concentration or molarity of a solution so 1 M = 1 mol/litre. A 1 M solution has 1 mole of the substance dissolved in 1 litre of solution. Square brackets arou ne symbol for the substance as in [Fe²*] are used to indicate concentration as molarity -see, for example, the way the Nernst equation is written.] Table 1. Standard Electrode Petential Standard Electrode Potential, V(V) Electrode Reaction Au + 3e O, + 4H + 4e 2H,0 Pr* + 2e Pt Ag* +e Ag Fe +e Fe* O, + 2H,0 + 4e 4(OH") Cu + 2e 2H* + 2e H; Pb + 2e - Pb Sn+ 2 - Sn N + 2e - Ni Co + 2e - Co Ca + 2e - Cd Fe* + 2e- Fe C + 3e- Cr Zn + 2e- AP + 3e- Al Mg+ + 2e-→ Mg Na* +e Na K* +e K - Au +1.420 +1.229 -+1.2 Increasingly inert (cathodic) +0.800 +0.771 +0.401 +0.340 Cu 0.000 -0.126 -0.136 -0.250 -0.277 -0.403 -0.440 -0.744 Increasingly active (anodic) - Zn --0.763 -1.662 -2.363 -2.714 -2.924 elect one: a. AVoltage is generated, AV = 0.04138 V, the iron electrode in the solution with the lower concentration of iron will oxidized. b. Voltage is generated, AV = 0.05283 V, the iron electrode in the solution with the higher concentration of iron will oxidized. c. Voltage is NOT generated. d. Voltage is generated, AV = 0.03128 V, the iron electrode in the solution with the higher concentration of iron will oxidized.

n electrochemical cell is constructed in which both electrodes are pure iron immersed in a solution of Fe ions. The [Fe1] concentration for one half cell is 0.5 M and [Fe2] for the other half cell is 0.02 he temperature of the solution is 25 °C. Is a voltage generated between the two half-cells? If so, what is its magnitude and which electrode will be oxidized? NOTE: The symbol M is used to indicate "molar" concentration or molarity of a solution so 1 M = 1 mol/litre. A 1 M solution has 1 mole of the substance dissolved in 1 litre of solution. Square brackets arou ne symbol for the substance as in [Fe²*] are used to indicate concentration as molarity -see, for example, the way the Nernst equation is written.] Table 1. Standard Electrode Petential Standard Electrode Potential, V(V) Electrode Reaction Au + 3e O, + 4H + 4e 2H,0 Pr* + 2e Pt Ag* +e Ag Fe +e Fe* O, + 2H,0 + 4e 4(OH") Cu + 2e 2H* + 2e H; Pb + 2e - Pb Sn+ 2 - Sn N + 2e - Ni Co + 2e - Co Ca + 2e - Cd Fe* + 2e- Fe C + 3e- Cr Zn + 2e- AP + 3e- Al Mg+ + 2e-→ Mg Na* +e Na K* +e K - Au +1.420 +1.229 -+1.2 Increasingly inert (cathodic) +0.800 +0.771 +0.401 +0.340 Cu 0.000 -0.126 -0.136 -0.250 -0.277 -0.403 -0.440 -0.744 Increasingly active (anodic) - Zn --0.763 -1.662 -2.363 -2.714 -2.924 elect one: a. AVoltage is generated, AV = 0.04138 V, the iron electrode in the solution with the lower concentration of iron will oxidized. b. Voltage is generated, AV = 0.05283 V, the iron electrode in the solution with the higher concentration of iron will oxidized. c. Voltage is NOT generated. d. Voltage is generated, AV = 0.03128 V, the iron electrode in the solution with the higher concentration of iron will oxidized.

Chemistry
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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An electrochemical cell is constructed in which both electrodes are pure iron immersed in a solution of Fe2+ ions. The [Fe12+] concentration for one half cell is 0.5 M and [Fez2+] for the other half cell is 0.02 M. The temperature of the solution is 25 °C. Is a voltage generated between the two half-cells? If so, what is its magnitude and which electrode will be oxidized? [NOTE: The symbol M is used to indicate "molar" concentration or molarity of a solution so 1 M = 1 mol/litre. A1M solution has 1 mole of the substance dissolved in 1 litre of solution. Square brackets around the symbol for the substance as in [Fe2*] are used to indicate concentration as molarity -see, for example, the way the Nernst equation is written.] Table 1. Standard Electrode Potentials Standard Electrode Potential, V°(V) Electrode Reaction Au+ + 3e O, + 4H* + 4e 2H,0 Pr2+ + 2e - Pt +1.420 +1.229 -+1.2 Au +0.800 Ag' + e - Ag Fe* + e - Fe* O, + 2H,0 + 4e + 4(OH") Cu²+ + 2e 2H* + 2e Pb* + 2e Pb Sn2+ + 2e Ni?* + 2e Ni Co+ + 2e - Co Cd+ + 2e Fe2+ + 2e Fe Cr* + 3e Cr Zn?+ + 2e AP+ + 3e Mg+ + 2e - Mg Na* +e - Na K* +e Increasingly inert (cathodic) +0.771 +0.401 +0.340 Cu 0.000 -0.126 --0.136 -0.250 -0.277 -0.403 → Sn -0.440 Increasingly active (anodic) --0.744 -0.763 -1.662 Zn Al -2.363 -2.714 - K -2.924 Select one: a. AVoltage is generated, AV = 0.04138 V, the iron electrode in the solution with the lower concentration of iron will oxidized. b. Voltage is generated, AV = 0.05283 V, the iron electrode in the solution with the higher concentration of iron will oxidized. c. Voltage is NOT generated. d. Voltage is generated, AV = 0.03128 V, the iron electrode in the solution with the higher concentration of iron will oxidized.
Transcribed Image Text:An electrochemical cell is constructed in which both electrodes are pure iron immersed in a solution of Fe2+ ions. The [Fe12+] concentration for one half cell is 0.5 M and [Fez2+] for the other half cell is 0.02 M. The temperature of the solution is 25 °C. Is a voltage generated between the two half-cells? If so, what is its magnitude and which electrode will be oxidized? [NOTE: The symbol M is used to indicate "molar" concentration or molarity of a solution so 1 M = 1 mol/litre. A1M solution has 1 mole of the substance dissolved in 1 litre of solution. Square brackets around the symbol for the substance as in [Fe2*] are used to indicate concentration as molarity -see, for example, the way the Nernst equation is written.] Table 1. Standard Electrode Potentials Standard Electrode Potential, V°(V) Electrode Reaction Au+ + 3e O, + 4H* + 4e 2H,0 Pr2+ + 2e - Pt +1.420 +1.229 -+1.2 Au +0.800 Ag' + e - Ag Fe* + e - Fe* O, + 2H,0 + 4e + 4(OH") Cu²+ + 2e 2H* + 2e Pb* + 2e Pb Sn2+ + 2e Ni?* + 2e Ni Co+ + 2e - Co Cd+ + 2e Fe2+ + 2e Fe Cr* + 3e Cr Zn?+ + 2e AP+ + 3e Mg+ + 2e - Mg Na* +e - Na K* +e Increasingly inert (cathodic) +0.771 +0.401 +0.340 Cu 0.000 -0.126 --0.136 -0.250 -0.277 -0.403 → Sn -0.440 Increasingly active (anodic) --0.744 -0.763 -1.662 Zn Al -2.363 -2.714 - K -2.924 Select one: a. AVoltage is generated, AV = 0.04138 V, the iron electrode in the solution with the lower concentration of iron will oxidized. b. Voltage is generated, AV = 0.05283 V, the iron electrode in the solution with the higher concentration of iron will oxidized. c. Voltage is NOT generated. d. Voltage is generated, AV = 0.03128 V, the iron electrode in the solution with the higher concentration of iron will oxidized.
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