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2. (20 pts) For the reaction Cu(s) + 2Ag+ (aq) → Cu2(aq) + 2Agos) a) Draw...
Consider the following electrochemical cell: Al (s) I Al3+ (aq) (1.00 M) II Cu2+ (aq) (0.0020...
Consider the following electrochemical cell: Al (s) I Al3+ (aq) (1.00 M) II Cu2+ (aq) (0.0020 M) I Cu (s) where Cu2+ aq + 2e- -> Cu (s) +0.34 V and Al3+ aq + 3e- -> Al (s) -1.66 V Calculate the standard cell potential for the given cell, calculate the cell potential for the given cell, and sketch the electrochemical cell using two beakers and labeling the electrodes, the cathode, the anode, the direction of electron flow in the...
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):
An electrochemical cell employs the reaction Mg2+(aq) + Cu(s) → Mg(s) + Cu2+(aq) and NaNO3 is...
An electrochemical cell employs the reaction Mg2+(aq) + Cu(s) → Mg(s) + Cu2+(aq) and NaNO3 is the salt used in the salt bridge. During the course of the reaction Na+ leaves the salt bridge and enters the anode compartment. NaNO3 leaves NaNO3 leaves the salt bridge and enters the anode compartment, the salt bridge and enters the anode compartment. Na+ leaves the salt bridge and enters the cathode compartment. NaNO3 leaves the salt bridge and enters the cathode compartment.
A galvanic cell employs the reaction Mg2+(aq) + Cu(s) → Mg(s) + Cu2+(aq) and NaNO3 is...
A galvanic cell employs the reaction Mg2+(aq) + Cu(s) → Mg(s) + Cu2+(aq) and NaNO3 is the salt used in the salt bridge. During the course of the reaction. A. NaNO3 leaves the salt bridge and enters the cathode compartment. B. Na+ leaves the salt bridge and enters the anode compartment. C. Na+ leaves the salt bridge and enters the cathode compartment. D. NaNO3 leaves the salt bridge and enters the anode compartment.
Consider the following voltaic cell: Sn(s) Sn2+ || Cu2+ Cu(s) Which metal is being oxidized? [Select]...
Consider the following voltaic cell: Sn(s) Sn2+ || Cu2+ Cu(s) Which metal is being oxidized? [Select] Which metal is being reduced? (Select] Identify and label the anode and cathode. anode (Select] cathode (Select] Salt bridge is made with potassium nitrate, show ion flow. [Select] Which electrode decreases in mass during cell operation? [Select] In which direction do electrons flow in the external circuit? [Select] At which electrode are electrons generated? [Select]
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) +...
A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are...
A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. 2Ag+ (aq) + Cu(s) + 2Ag(s) + Cu2+ (aq) The anode reaction is: The cathode reaction is: + In the external circuit, electrons migrate the Ag|Ag+ electrode the Cu Cu2+ electrode. In the salt bridge, anions migrate the CuCu2+ compartment the Ag|Ag compartment.
For the reaction Cu (s) + 2Ag+ (aq) Cu2+ (aq) + 2Ag (s) at 25 °C, the...
For the reaction Cu (s) + 2Ag+ (aq) Cu2+ (aq) + 2Ag (s) at 25 °C, the cell potential is found to be 0.62 V. Everything is at standard state except the Cu2+ (aq). Calculate [Cu2+].
3. Consider the following voltaic cell: Sn(s) Sn2+ || Cu2+ Cu(s) Answer: read 21.2, see sample...
3. Consider the following voltaic cell: Sn(s) Sn2+ || Cu2+ Cu(s) Answer: read 21.2, see sample problem 21.2 A. Which metal is being oxidized? B. Which metal is being reduced? C. Identify and label the anode/cathode/salt bridge D. Salt bridge is made with potassium nitrate, show ion flow E. Which electrode decreases in mass during cell operation? F. In which direction do electrons flow in the external circuit? G. At which electrode are electrons generated?
Draw the diagram for the standard cell potential of a Cu/Cu cell that is 0.05 M...
Draw the diagram for the standard cell potential of a Cu/Cu cell that is 0.05 M and 1.00 M in cusoa. Label the anode, cathode, direction of electron flow, salt bridge, oxidation side, and reducing side. 1.
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):
An electrochemical cell employs the reaction Mg2+(aq) + Cu(s) → Mg(s) + Cu2+(aq) and NaNO3 is the salt used in the salt bridge. During the course of the reaction Na+ leaves the salt bridge and enters the anode compartment. NaNO3 leaves NaNO3 leaves the salt bridge and enters the anode compartment, the salt bridge and enters the anode compartment. Na+ leaves the salt bridge and enters the cathode compartment. NaNO3 leaves the salt bridge and enters the cathode compartment.
Consider the following voltaic cell: Sn(s) Sn2+ || Cu2+ Cu(s) Which metal is being oxidized? [Select] Which metal is being reduced? (Select] Identify and label the anode and cathode. anode (Select] cathode (Select] Salt bridge is made with potassium nitrate, show ion flow. [Select] Which electrode decreases in mass during cell operation? [Select] In which direction do electrons flow in the external circuit? [Select] At which electrode are electrons generated? [Select]
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) +...
A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. 2Ag+ (aq) + Cu(s) + 2Ag(s) + Cu2+ (aq) The anode reaction is: The cathode reaction is: + In the external circuit, electrons migrate the Ag|Ag+ electrode the Cu Cu2+ electrode. In the salt bridge, anions migrate the CuCu2+ compartment the Ag|Ag compartment.
3. Consider the following voltaic cell: Sn(s) Sn2+ || Cu2+ Cu(s) Answer: read 21.2, see sample problem 21.2 A. Which metal is being oxidized? B. Which metal is being reduced? C. Identify and label the anode/cathode/salt bridge D. Salt bridge is made with potassium nitrate, show ion flow E. Which electrode decreases in mass during cell operation? F. In which direction do electrons flow in the external circuit? G. At which electrode are electrons generated?
Draw the diagram for the standard cell potential of a Cu/Cu cell that is 0.05 M and 1.00 M in cusoa. Label the anode, cathode, direction of electron flow, salt bridge, oxidation side, and reducing side. 1.
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