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)
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Chapter1: Chemical Foundations
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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)
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