d. Which specie Can be oxidized by Mno in acid? 1. Consider a simple galvanic cell consisting of two beakers connected by a salt bridge. One beaker contains a solution of Mno, in dilute sulfuric acid and has a Pt electrode. The other beaker contains a solution of Sn²* in dilute sulphuric acid, also with a Pt electrode. When the two electrodes are connected by a wire, current flows and a spontaneous reaction occurs that is described by the following balanced chemical equation: 2Mnoag) + 5Sn2+ (ag) + 16H* (ng) - 2Mn2* (ag) + 5Sn** (ag) + 8H,00 For this galvanic cell, a. Write the half - reaction that occurs at each electrode b. Indicate which electrode is the cathode and which is the anode C. Indicate which electrode is the positive electrode and which is the negative electrode The ha 2. Draw the cell diagram for the following reaction, assuming the concentration of Ag* and Mg are each 1M Mg + 2Ag* (ag) Mg (eg) + 2Ag) 3. Consider only the species (at standard conditions), in answering the following questions. Give reason for your answers. (Use data from the Standard Reduction Potential table) Br", Brz, H*, Hz, La, Ca and cd a. Which is the strongest axidizing agent? b. Which is the strongest reducing agent? C. Which species can be reduced by Zn(s)? 4. Sketch the galvanic cell based on the following overall reactions. Calculate ; show the direction of clectron flow and the direction of ion migration through the salt bridge; identify the cathode and anode: and give the overall balanced reaction. Assume that all concentrations are 1.0 M and that all partiei pressures are 1.0 atm. Refer to the table above for the standard reduction potential a. Cr* (ag) + CI,(G) = Cr,0 (aq) + Cr b. Cu?+(aq) + Mg(5) =t Mg (aq) + Cu(s) c.105 (ag) + Pe (aq) Pe* Caq) + (s) d. Zn(s) + Ag*(aq) Zn* (aq) +Agls)
d. Which specie Can be oxidized by Mno in acid? 1. Consider a simple galvanic cell consisting of two beakers connected by a salt bridge. One beaker contains a solution of Mno, in dilute sulfuric acid and has a Pt electrode. The other beaker contains a solution of Sn²* in dilute sulphuric acid, also with a Pt electrode. When the two electrodes are connected by a wire, current flows and a spontaneous reaction occurs that is described by the following balanced chemical equation: 2Mnoag) + 5Sn2+ (ag) + 16H* (ng) - 2Mn2* (ag) + 5Sn** (ag) + 8H,00 For this galvanic cell, a. Write the half - reaction that occurs at each electrode b. Indicate which electrode is the cathode and which is the anode C. Indicate which electrode is the positive electrode and which is the negative electrode The ha 2. Draw the cell diagram for the following reaction, assuming the concentration of Ag* and Mg are each 1M Mg + 2Ag* (ag) Mg (eg) + 2Ag) 3. Consider only the species (at standard conditions), in answering the following questions. Give reason for your answers. (Use data from the Standard Reduction Potential table) Br", Brz, H*, Hz, La, Ca and cd a. Which is the strongest axidizing agent? b. Which is the strongest reducing agent? C. Which species can be reduced by Zn(s)? 4. Sketch the galvanic cell based on the following overall reactions. Calculate ; show the direction of clectron flow and the direction of ion migration through the salt bridge; identify the cathode and anode: and give the overall balanced reaction. Assume that all concentrations are 1.0 M and that all partiei pressures are 1.0 atm. Refer to the table above for the standard reduction potential a. Cr* (ag) + CI,(G) = Cr,0 (aq) + Cr b. Cu?+(aq) + Mg(5) =t Mg (aq) + Cu(s) c.105 (ag) + Pe (aq) Pe* Caq) + (s) d. Zn(s) + Ag*(aq) Zn* (aq) +Agls)
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 77AP
Related questions
Question
Questions attached
Transcribed Image Text:d. Which specie Can be oxidized by Mno in acid?
1. Consider a simple galvanic cell consisting of two beakers connected by a salt bridge. One beaker
contains a solution of Mno, in dilute sulfuric acid and has a Pt electrode. The other beaker contains
a solution of Sn²* in dilute sulphuric acid, also with a Pt electrode. When the two electrodes are
connected by a wire, current flows and a spontaneous reaction occurs that is described by the
following balanced chemical equation:
2Mnoag) + 5Sn2+ (ag) + 16H* (ng) - 2Mn2* (ag) + 5Sn** (ag) + 8H,00
For this galvanic cell,
a. Write the half - reaction that occurs at each electrode
b. Indicate which electrode is the cathode and which is the anode
C. Indicate which electrode is the positive electrode and which is the negative electrode
The ha
2. Draw the cell diagram for the following reaction, assuming the concentration of Ag* and Mg are each
1M
Mg + 2Ag* (ag) Mg (eg) + 2Ag)
3. Consider only the species (at standard conditions), in answering the following questions. Give reason
for your answers. (Use data from the Standard Reduction Potential table)
Br", Brz, H*, Hz, La, Ca and cd
a. Which is the strongest axidizing agent?
b. Which is the strongest reducing agent?
C. Which species
can be reduced by Zn(s)?
4. Sketch the galvanic cell based on the following overall reactions. Calculate ; show the direction of
clectron flow and the direction of ion migration through the salt bridge; identify the cathode and anode:
and give the overall balanced reaction. Assume that all concentrations are 1.0 M and that all partiei
pressures are 1.0 atm. Refer to the table above for the standard reduction potential
a. Cr* (ag) + CI,(G) = Cr,0 (aq) + Cr
b. Cu?+(aq) + Mg(5) =t Mg (aq) + Cu(s)
c.105 (ag) + Pe (aq) Pe* Caq) + (s)
d. Zn(s) + Ag*(aq) Zn* (aq) +Agls)
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 3 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
