The salt bridge was soaked with a saturated solution of KNO3. In which direction do the...
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The
salt bridge was soaked with a saturated solution of KNO3. In which
direction do the...
Post-Laboratory Report (Page 1/1) Group Number Date: Day Time 1. The salt bridge in Goal #1 was s...
Post-Laboratory Report (Page 1/1) Group Number Date: Day Time 1. The salt bridge in Goal #1 was soaked with a saturated ammonium nitrate solution. In which direction do the ammonium ions move when this salt bridge completed the electric circuit? Toward the zinc metal or toward the copper metal? In which direction do the nitrate ions move? 2. In a concentration cell, what would be the potential if we studied two solutions that had the same concentration? Show that the...
20. Which one of the following reactions is spontaneous (in the direction given) under standard e...
Please answer the following questions!
20. Which one of the following reactions is spontaneous (in the direction given) under standard electrochemical conditions? +2Br- Mg+ Br2 What is the cell potential for a cell constructed by immersing a strip of manganese in a 1. M MnSO4 solution and a strip of iron in a 1.0 M FesO4 solution and completing the circuit by a wire and a salt bridge? 21. b. +1.62 V c. -0.74 V d. +0.74 V e. +1.21...
In a copper-zinc voltaic cell, one half-cell consists of a ZnZn electrode inserted in a solution...
In a copper-zinc voltaic cell, one half-cell consists of a ZnZn
electrode inserted in a solution of zinc sulfate and the other
half-cell consists of a CuCu electrode inserted in a copper sulfate
solution. These two half-cells are separated by a salt bridge.
At the zinc electrode (anode), ZnZn metal undergoes oxidation by
losing two electrons and enters the solution as Zn2+Zn2+ ions. The
oxidation half-cell reaction that takes place at the anode is
Zn(s)→Zn2+(aq)+2e−Zn(s)→Zn2+(aq)+2e−
The CuCu ions undergo reduction...
Name Date Class The Electrochemical Cell salt bridge 10N U ANNO, 1.0M Pb(NO), Answer the questions...
Name Date Class The Electrochemical Cell salt bridge 10N U ANNO, 1.0M Pb(NO), Answer the questions below referring to the above diagram. 1. Which is more easily oxidized metal, aluminum or lead? What is the balanced equation showing the spontaneous reaction that occurs? What is the direction of electron flow in the wire? What is the direction of positive ion flow in the salt bridge? What is happening to the concentration of aluminum ions? What is happening to the concentration...
salt bridge Zn(s) electrode Culs) electrode 1.0M Zn (a 1.0 M Cu (aq A voltaic cell...
salt bridge Zn(s) electrode Culs) electrode 1.0M Zn (a 1.0 M Cu (aq A voltaic cell similar to that shown in the figure above is constructed. The electronic device shown at the top of the figure is a volt meter. One electrode compartment consists of a zinc strip placed in a 1.0 M ZnCl2 solution, and the other has a copper strip placed in a 1.0 M CuSOA solution. The overall cell reaction is: Zn(s)Cu2+(aq)= zn2+ (aq ) Cu (s)...
The CuCu ions undergo reduction by accepting two electrons from the copper electrode (cathode) and depositing...
The CuCu ions undergo reduction by accepting two electrons from
the copper electrode (cathode) and depositing on the electrode as
Cu(s)Cu(s). The reduction half-cell reaction that takes place at
the cathode is
Cu^2+(aq)+2e^−→Cu(s)Cu^2+(aq)+2e^-→Cu(s)
The electrons lost by the ZnZn metal are gained by the CuCu ion.
The transfer of electrons between ZnZn metal and CuCu ions is made
possible by connecting the wire between the ZnZn electrode and the
CuCu electrode. Thus, in the voltaic cell, the electrons flow
through...
salt bridge ME Cr(s) electrode Cu(s) electrode 1.0 M Cr3+ (aq) 1.0 M Cu2+ (aq) A...
salt bridge ME Cr(s) electrode Cu(s) electrode 1.0 M Cr3+ (aq) 1.0 M Cu2+ (aq) A electrolytic cell similar to that shown in the figure above is constructed. The electronic device shown at the top of the figure is a power supply. One electrode compartment consists of a chromium strip placed in a 1.0 M CrCl3 solution, and the other has a copper strip placed in a 1.0 M CuSO4 solution. The overall cell reaction is: 2 Cr3+ (aq) +...
Choose the label which best describes the following: A B C D E F G H Direction...
Choose the label which best describes the following:
A B C D E F G H Direction which anions move through the
salt bridge
A B C D E F G H Pt anode
The overall, balanced, spontaneous reaction occurring in this
(standard) cell is:
Cr2O72−(aq) + 6Cl−(aq)
+ 14H+(aq) → 7H2O(l) + 2Cr3+(aq) +
3Cl2(g)
7H2O(l) + 2Cr3+(aq) + 3Cl2(g) →
Cr2O72−(aq) + 6Cl−(aq)
+ 14H+(aq)
7H2O(l) + 2Cr3+(aq) + Cl2(g) →
Cr2O72−(aq) + 2Cl−(aq)
+ 14H+(aq)
2Cr3+(aq) + 3Cl2(g) →...
(a) Write the Nernst equations for the half-reactions in Demonstration 14 - 1. In which direction...
(a) Write the Nernst equations for the half-reactions in
Demonstration 14 - 1. In which direction do electrons move through
the circuit? (b) If you use your fingers as a salt bridge in
Demonstration 14-1, will your body take in Cu2+ or Zn2+?
pH ete Reference electrode socket Glass electrode socket Salt bridge Strip of Zn metal 0.1 M L ZnCl2 0.1 M CuSO4 Strip of Cu metal
5. What was the purpose of the NaNO3 solution in this experiment? 6. Could a solution...
5. What was the purpose of the NaNO3 solution in this experiment? 6. Could a solution of NaCl be used instead of NaNO3? 7. What was the purpose of FeSO4 solution in this experiment? 8. Could a solution of FeCl, be used instead of FeSO4? 9. Could a solution of NaSO4 be used instead of FeSO4? 10. Calculate the standard cell potential for the spontaneous redox reaction between a Pb(s)/Pb(NO3)2(aq) half-cell and a Ag(s)/AgNO3(aq) half-cell. Which metal would be oxidized?...
Post-Laboratory Report (Page 1/1) Group Number Date: Day Time 1. The salt bridge in Goal #1 was soaked with a saturated ammonium nitrate solution. In which direction do the ammonium ions move when this salt bridge completed the electric circuit? Toward the zinc metal or toward the copper metal? In which direction do the nitrate ions move? 2. In a concentration cell, what would be the potential if we studied two solutions that had the same concentration? Show that the...
Please answer the following questions!
20. Which one of the following reactions is spontaneous (in the direction given) under standard electrochemical conditions? +2Br- Mg+ Br2 What is the cell potential for a cell constructed by immersing a strip of manganese in a 1. M MnSO4 solution and a strip of iron in a 1.0 M FesO4 solution and completing the circuit by a wire and a salt bridge? 21. b. +1.62 V c. -0.74 V d. +0.74 V e. +1.21...
In a copper-zinc voltaic cell, one half-cell consists of a ZnZn
electrode inserted in a solution of zinc sulfate and the other
half-cell consists of a CuCu electrode inserted in a copper sulfate
solution. These two half-cells are separated by a salt bridge.
At the zinc electrode (anode), ZnZn metal undergoes oxidation by
losing two electrons and enters the solution as Zn2+Zn2+ ions. The
oxidation half-cell reaction that takes place at the anode is
Zn(s)→Zn2+(aq)+2e−Zn(s)→Zn2+(aq)+2e−
The CuCu ions undergo reduction...
Name Date Class The Electrochemical Cell salt bridge 10N U ANNO, 1.0M Pb(NO), Answer the questions below referring to the above diagram. 1. Which is more easily oxidized metal, aluminum or lead? What is the balanced equation showing the spontaneous reaction that occurs? What is the direction of electron flow in the wire? What is the direction of positive ion flow in the salt bridge? What is happening to the concentration of aluminum ions? What is happening to the concentration...
salt bridge Zn(s) electrode Culs) electrode 1.0M Zn (a 1.0 M Cu (aq A voltaic cell similar to that shown in the figure above is constructed. The electronic device shown at the top of the figure is a volt meter. One electrode compartment consists of a zinc strip placed in a 1.0 M ZnCl2 solution, and the other has a copper strip placed in a 1.0 M CuSOA solution. The overall cell reaction is: Zn(s)Cu2+(aq)= zn2+ (aq ) Cu (s)...
The CuCu ions undergo reduction by accepting two electrons from
the copper electrode (cathode) and depositing on the electrode as
Cu(s)Cu(s). The reduction half-cell reaction that takes place at
the cathode is
Cu^2+(aq)+2e^−→Cu(s)Cu^2+(aq)+2e^-→Cu(s)
The electrons lost by the ZnZn metal are gained by the CuCu ion.
The transfer of electrons between ZnZn metal and CuCu ions is made
possible by connecting the wire between the ZnZn electrode and the
CuCu electrode. Thus, in the voltaic cell, the electrons flow
through...
salt bridge ME Cr(s) electrode Cu(s) electrode 1.0 M Cr3+ (aq) 1.0 M Cu2+ (aq) A electrolytic cell similar to that shown in the figure above is constructed. The electronic device shown at the top of the figure is a power supply. One electrode compartment consists of a chromium strip placed in a 1.0 M CrCl3 solution, and the other has a copper strip placed in a 1.0 M CuSO4 solution. The overall cell reaction is: 2 Cr3+ (aq) +...
Choose the label which best describes the following:
A B C D E F G H Direction which anions move through the
salt bridge
A B C D E F G H Pt anode
The overall, balanced, spontaneous reaction occurring in this
(standard) cell is:
Cr2O72−(aq) + 6Cl−(aq)
+ 14H+(aq) → 7H2O(l) + 2Cr3+(aq) +
3Cl2(g)
7H2O(l) + 2Cr3+(aq) + 3Cl2(g) →
Cr2O72−(aq) + 6Cl−(aq)
+ 14H+(aq)
7H2O(l) + 2Cr3+(aq) + Cl2(g) →
Cr2O72−(aq) + 2Cl−(aq)
+ 14H+(aq)
2Cr3+(aq) + 3Cl2(g) →...
(a) Write the Nernst equations for the half-reactions in
Demonstration 14 - 1. In which direction do electrons move through
the circuit? (b) If you use your fingers as a salt bridge in
Demonstration 14-1, will your body take in Cu2+ or Zn2+?
pH ete Reference electrode socket Glass electrode socket Salt bridge Strip of Zn metal 0.1 M L ZnCl2 0.1 M CuSO4 Strip of Cu metal
5. What was the purpose of the NaNO3 solution in this experiment? 6. Could a solution of NaCl be used instead of NaNO3? 7. What was the purpose of FeSO4 solution in this experiment? 8. Could a solution of FeCl, be used instead of FeSO4? 9. Could a solution of NaSO4 be used instead of FeSO4? 10. Calculate the standard cell potential for the spontaneous redox reaction between a Pb(s)/Pb(NO3)2(aq) half-cell and a Ag(s)/AgNO3(aq) half-cell. Which metal would be oxidized?...
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