PLEASE DON'T BE INTIMIDATED BY HOW LONG THIS IS! JUST ANSWER THE MOST YOU CAN :)
These are chapter 19 Review Questions in Modern Chemistry Texbook:
22. If a strip of Ni were dipped into a solution of AgNO3,whatt would be expected to occur? Explain, using E^0 values.
23. a. What would happen if an aluminum spoon were used to stir a solution of Zn(NO3)2?
b. Could a strip of Zn be used to stir a solution of Al(NO3)3?
31. A voltaic cell is made up of a cadmium electrode in a solution of CdSO4 and a zinc electrode in a solution of ZnSO4. The two half-cells are separated by a prous barrier.
a. What is the cathode, and which is the anode?
b. In which direction are the electrons flowing?
c. Write balanced equations for the two half-reactions, and write a net equation for the combined reaction.
These areSupplementt Questions:
S3) A cell is based on the reaction
Ni(s) + 2Ag+(aq) = Ni2+(aq) + 2Ag(s)
What would be the effect on the cell voltage if:
a.) some AgNO3 was dissolved into the solution around the silver electrode
b.) some NiSO4 was dissolved into the solution around the nickel electrode
c.) Ag2S was precipitated out of the system by adding H2S to the Ag+/Ag(s) half of the cell?
S4) The E^0 value for the half-reaction
Ag(s) = Ag+(aq) + e-
as written is -0.80 volt. What would happen to the measured half-cell value (H+/H2 reference) if a salt solution (NaCl) was added to the solution around the silver electrode?
Which one of the following values would be most reasonable:
-0.40
-0.80
-1.20
Explain your answer
These are chapter 19 Review Questions in Modern Chemistry Texbook:
22. If a strip of Ni were dipped into a solution of AgNO3,whatt would be expected to occur? Explain, using E^0 values.
23. a. What would happen if an aluminum spoon were used to stir a solution of Zn(NO3)2?
b. Could a strip of Zn be used to stir a solution of Al(NO3)3?
31. A voltaic cell is made up of a cadmium electrode in a solution of CdSO4 and a zinc electrode in a solution of ZnSO4. The two half-cells are separated by a prous barrier.
a. What is the cathode, and which is the anode?
b. In which direction are the electrons flowing?
c. Write balanced equations for the two half-reactions, and write a net equation for the combined reaction.
These areSupplementt Questions:
S3) A cell is based on the reaction
Ni(s) + 2Ag+(aq) = Ni2+(aq) + 2Ag(s)
What would be the effect on the cell voltage if:
a.) some AgNO3 was dissolved into the solution around the silver electrode
b.) some NiSO4 was dissolved into the solution around the nickel electrode
c.) Ag2S was precipitated out of the system by adding H2S to the Ag+/Ag(s) half of the cell?
S4) The E^0 value for the half-reaction
Ag(s) = Ag+(aq) + e-
as written is -0.80 volt. What would happen to the measured half-cell value (H+/H2 reference) if a salt solution (NaCl) was added to the solution around the silver electrode?
Which one of the following values would be most reasonable:
-0.40
-0.80
-1.20
Explain your answer
-
reduction potential of Ag+ = 0.8V
reduction potential of Ni2+ = -0.25V so the oxidation potential of Ni 2+ = 0.25V
Ni is more reactive than Ag so Ni will replace the Ag in AgNO3
the reduction potential of Ag+ > Ni2+, Ag+ will be reduced
Al + Zn(NO3)2 --> Al(NO3)3 + Znº
Zn will not replace Al since Al is more reactive than Zn
reduction potential for Zn 2+ = -0.76
reduction potential for Cd 2+ = -0.4
Zn is more likely to be oxidized so this is the anode, Cd = cathode
electrons flow through the anode to the cathode. if the anode is the oxidation site, electrons will move off of the anode and gather at the cathode.
Zn --> Zn 2+ + 2e-
Cd 2+ + 2e- --> Cd
addition of AgNO3 would provide more Ag+ oxidation of Ni would occur more voltage increases
adding NiSO4 would drop the voltage since Ni 2+ would already be in the system, oxidation of Ni would slow or stop
adding H2S forming Ag2S would slow and stop the oxidation of Ni, voltage would drop
oxidation potential = -0.8
?
reduction potential of Ni2+ = -0.25V so the oxidation potential of Ni 2+ = 0.25V
Ni is more reactive than Ag so Ni will replace the Ag in AgNO3
the reduction potential of Ag+ > Ni2+, Ag+ will be reduced
Al + Zn(NO3)2 --> Al(NO3)3 + Znº
Zn will not replace Al since Al is more reactive than Zn
reduction potential for Zn 2+ = -0.76
reduction potential for Cd 2+ = -0.4
Zn is more likely to be oxidized so this is the anode, Cd = cathode
electrons flow through the anode to the cathode. if the anode is the oxidation site, electrons will move off of the anode and gather at the cathode.
Zn --> Zn 2+ + 2e-
Cd 2+ + 2e- --> Cd
addition of AgNO3 would provide more Ag+ oxidation of Ni would occur more voltage increases
adding NiSO4 would drop the voltage since Ni 2+ would already be in the system, oxidation of Ni would slow or stop
adding H2S forming Ag2S would slow and stop the oxidation of Ni, voltage would drop
oxidation potential = -0.8
?