A voltaic cell (also called a galvanic cell) was constructed by connecting two beakers with a salt bridge. In one beaker, an iron plate was immersed in a 1 M solution of iron(II) nitrate, Fe(NO3)2. In the other beaker, a lead plate was immersed in a 1 M solution of lead(II) nitrate, Pb(NO3)2. What voltage is generated by this cell under standard conditions at 25 oC? Note the following standard half-cell reduction potentials: Fe2+(aq) + 2e- -----> Fe(s) Eo = -0.45 V Pb2+(aq) + 2e- -----> Pb(s) Eo = -0.13 V In the voltaic cell described previously, which consists of iron and lead plates, each immersed in a 1 M solution of their respective ions, which beaker contains the anode? Group of answer choices The beaker with the lead plate. The beaker with the iron plate. Consider again, the voltaic cell described previously, that consists of iron and lead plates, each immersed in a 1 M solution of their respective ions. Based on the standard cell voltage that you calculated for this cell, what is DGo for the redox reaction that takes place in this cell? Note that the Farady constant is 96485 Coulomb/mol. -322 kJ -155 kJ -62 kJ -14 kJ 31 kJ
A voltaic cell (also called a galvanic cell) was constructed by connecting two beakers with a salt bridge. In one beaker, an iron plate was immersed in a 1 M solution of iron(II) nitrate, Fe(NO3)2. In the other beaker, a lead plate was immersed in a 1 M solution of lead(II) nitrate, Pb(NO3)2. What voltage is generated by this cell under standard conditions at 25 oC? Note the following standard half-cell reduction potentials: Fe2+(aq) + 2e- -----> Fe(s) Eo = -0.45 V Pb2+(aq) + 2e- -----> Pb(s) Eo = -0.13 V In the voltaic cell described previously, which consists of iron and lead plates, each immersed in a 1 M solution of their respective ions, which beaker contains the anode? Group of answer choices The beaker with the lead plate. The beaker with the iron plate. Consider again, the voltaic cell described previously, that consists of iron and lead plates, each immersed in a 1 M solution of their respective ions. Based on the standard cell voltage that you calculated for this cell, what is DGo for the redox reaction that takes place in this cell? Note that the Farady constant is 96485 Coulomb/mol. -322 kJ -155 kJ -62 kJ -14 kJ 31 kJ
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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A voltaic cell (also called a galvanic cell) was constructed by connecting two beakers with a salt bridge. In one beaker, an iron plate was immersed in a 1 M solution of iron(II) nitrate, Fe(NO3)2. In the other beaker, a lead plate was immersed in a 1 M solution of lead(II) nitrate, Pb(NO3)2. What voltage is generated by this cell under standard conditions at 25 oC? Note the following standard half-cell reduction potentials:
Fe2+(aq) + 2e- -----> Fe(s) Eo = -0.45 V
Pb2+(aq) + 2e- -----> Pb(s) Eo = -0.13 V
In the voltaic cell described previously, which consists of iron and lead plates, each immersed in a 1 M solution of their respective ions, which beaker contains the anode?
Group of answer choices
The beaker with the lead plate.
The beaker with the iron plate.
Consider again, the voltaic cell described previously, that consists of iron and lead plates, each immersed in a 1 M solution of their respective ions. Based on the standard cell voltage that you calculated for this cell, what is DGo for the redox reaction that takes place in this cell? Note that the Farady constant is 96485 Coulomb/mol.
-322 kJ
-155 kJ
-62 kJ
-14 kJ
31 kJ
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