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3. Draw a functional Galvanic cell given the following: Co Co + 2 e and Cu...
Consider the galvanic cell that uses the reaction 2 Ag^+ (aq) + Cu(s) rightarrow Cu^2+ (aq)...
Consider the galvanic cell that uses the reaction 2 Ag^+ (aq) + Cu(s) rightarrow Cu^2+ (aq) + 2 Ag (s) Clearly sketch the experimental set-up, write down the anode and cathode half-reactions, and give the shorthand notation for the cell.
7. You decide to construct a zinc/aluminum galvanic cell in which the electrodes are connected by...
7. You decide to construct a zinc/aluminum galvanic cell in which the electrodes are connected by a wire and the solutions are connected with a salt bridge. One electrode consists of an aluminum bar in a 1.0 M solution of aluminum nitrate. The other electrode consists of zinc bar in a 1.0 M solution of zinc nitrate. Draw the complete electrochemical cell diagram and use it to answer the questions that follow. a. Which electrode is the cathode and which...
V. Concentration Cell Copper - Copper Cy(s), CuCl2 (0.01) || Cu(s), CuCl2 (1.0 M) 1. Draw...
V. Concentration Cell Copper - Copper Cy(s), CuCl2 (0.01) || Cu(s), CuCl2 (1.0 M) 1. Draw the schematic of the electrochemical cell that includes all the components (metals, solutions, salt bridges, voltmeters, etc.). Annotate on the schematic which side is the anode, which side is the cathode, the sign of each half cell, the composition of the metals and solutions, and the direction of the flow of the electrons through the cell. 2. Write the half reactions that occur at...
Constants The following values may be useful when solving this tutorial. Constant E°Cu | 0.337V E°Co...
Constants The following values may be useful when solving this tutorial. Constant E°Cu | 0.337V E°Co | -0.277V R. | 8.314 J•mol^-1•K^-1 F | 96485 C/mol T. | 298 K In the activity, click on the E°cell and Keq quantities to observe how they are related. Use this relation to calculate Keq for the following redox reaction that occurs in an electrochemical cell having two electrodes: a cathode and an anode. The two half-reactions that occurs in the cell are...
Part A through H 1. [60 pts) A galvanic cell is a type of battery where...
Part A through H
1. [60 pts) A galvanic cell is a type of battery where the electrodes are immersed in different electrolyte solutions, which are connected by an ion-conducting bridge. Consider a galvanic cell with Al and Cu electrodes. The Al electrode is immersed in a solution containing a standard concentration of Al3+ ions and the Cu electrode is immersed in a solution containing a standard concentration of Cu* ions. External Circuit The standard reduction potentials for the half...
please show all work. thank you 4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic...
please show all work. thank you
4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic cell) with Ag(s) and 1.0 M AgNO3(aq) in one compartment and Cu(s) and 1.0 M Cu(NO3)2(aq) in the other compartment. Write the reactions and calculate the standard state cell potential at 298 K. E cathode = a. Reduction (cathode): Eanode = b. Oxidation (anode): Eºcell = C. Net (overall cell reaction): 5. Consider a galvanic cell with Sn(s) and 1.0 M Sn(NO3)2(aq) in one...
data collected Cu(NO3)2 | Zn(NO3)2 = 0.999 V Pb | 1.0 M Pb(NO3)2 || 1.0 M...
data collected
Cu(NO3)2 | Zn(NO3)2 = 0.999 V
Pb | 1.0 M Pb(NO3)2 || 1.0 M Zn(NO3)2 | Zn = 0.396 V
PART B: REDUCTION POTENTIALS 1. Report the measured cell potential for each galvanic cell and state which electrode corresponds to the cathode and which to the anode. 2. Given E = -0.76 V for the Zn/Zn half-cell, and your measured Ecell, calculate the reduction potential at the Cu and Pb electrodes and write the redox half- 6 reactions...
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that...
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that the transfer of electrons is forced to occur across a wire. The resulting electricity is measured in volts (V) and is the sum of the potentials of the oxidation and reduction half-reactions: E^o cell = E^o red + E^o ox By reversing the reduction half-reactions, you get the corresponding oxidation half-reaction, for which E^o ox has the opposite sign of E^o red You can...
Suppose the galvanic cell sketched below is powered by the following reaction: Cu(s)+2 AgNO3(aq) → Cu(NO3),...
Suppose the galvanic cell sketched below is powered by the following reaction: Cu(s)+2 AgNO3(aq) → Cu(NO3), (29)+2 Ag(s) Write a balanced equation for the half-reaction that happens at the cathode of this cell. 0-0 Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is El made? xs ? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution SZ?
On the cell diagram, label (9 pts): • the electrodes (Cr & Cu) • each aqueous...
On the cell diagram, label (9 pts): • the electrodes (Cr & Cu) • each aqueous solution (Cr(NO3); KNO3; Cu(NO3)2) • anode & cathode • salt bridge (including ions) • the (+) and (-) terminus the direction of electron flow movement of ALL ions where is oxidation occurring, show the process where is reduction occurring, show the process Write the short-hand cell notation (2 pts):
Consider the galvanic cell that uses the reaction 2 Ag^+ (aq) + Cu(s) rightarrow Cu^2+ (aq) + 2 Ag (s) Clearly sketch the experimental set-up, write down the anode and cathode half-reactions, and give the shorthand notation for the cell.
7. You decide to construct a zinc/aluminum galvanic cell in which the electrodes are connected by a wire and the solutions are connected with a salt bridge. One electrode consists of an aluminum bar in a 1.0 M solution of aluminum nitrate. The other electrode consists of zinc bar in a 1.0 M solution of zinc nitrate. Draw the complete electrochemical cell diagram and use it to answer the questions that follow. a. Which electrode is the cathode and which...
Part A through H
1. [60 pts) A galvanic cell is a type of battery where the electrodes are immersed in different electrolyte solutions, which are connected by an ion-conducting bridge. Consider a galvanic cell with Al and Cu electrodes. The Al electrode is immersed in a solution containing a standard concentration of Al3+ ions and the Cu electrode is immersed in a solution containing a standard concentration of Cu* ions. External Circuit The standard reduction potentials for the half...
please show all work. thank you
4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic cell) with Ag(s) and 1.0 M AgNO3(aq) in one compartment and Cu(s) and 1.0 M Cu(NO3)2(aq) in the other compartment. Write the reactions and calculate the standard state cell potential at 298 K. E cathode = a. Reduction (cathode): Eanode = b. Oxidation (anode): Eºcell = C. Net (overall cell reaction): 5. Consider a galvanic cell with Sn(s) and 1.0 M Sn(NO3)2(aq) in one...
data collected
Cu(NO3)2 | Zn(NO3)2 = 0.999 V
Pb | 1.0 M Pb(NO3)2 || 1.0 M Zn(NO3)2 | Zn = 0.396 V
PART B: REDUCTION POTENTIALS 1. Report the measured cell potential for each galvanic cell and state which electrode corresponds to the cathode and which to the anode. 2. Given E = -0.76 V for the Zn/Zn half-cell, and your measured Ecell, calculate the reduction potential at the Cu and Pb electrodes and write the redox half- 6 reactions...
In a galvanic cell, a spontaneous redox reaction occurs. However the reactants are separated such that the transfer of electrons is forced to occur across a wire. The resulting electricity is measured in volts (V) and is the sum of the potentials of the oxidation and reduction half-reactions: E^o cell = E^o red + E^o ox By reversing the reduction half-reactions, you get the corresponding oxidation half-reaction, for which E^o ox has the opposite sign of E^o red You can...
Suppose the galvanic cell sketched below is powered by the following reaction: Cu(s)+2 AgNO3(aq) → Cu(NO3), (29)+2 Ag(s) Write a balanced equation for the half-reaction that happens at the cathode of this cell. 0-0 Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is El made? xs ? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution SZ?
On the cell diagram, label (9 pts): • the electrodes (Cr & Cu) • each aqueous solution (Cr(NO3); KNO3; Cu(NO3)2) • anode & cathode • salt bridge (including ions) • the (+) and (-) terminus the direction of electron flow movement of ALL ions where is oxidation occurring, show the process where is reduction occurring, show the process Write the short-hand cell notation (2 pts):
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