Consider the following unbalanced equation.
Ag1+ (aq) + Cu (s) Ag (s) + Cu2+ (aq)
Type the following answers using the formats given. Use only the format '1+' or '1-' for the charge on an ion. If only one electron is present in the half-cell reaction, type the answer as e- instead of 1e-.
Half-cell Equation Au3+(aq) + 3 e- Au(s)
Typed Answer Au3+(aq) + 3e- > Au(s)
Balanced Equation 2 Au3+(aq) + 3 Zn(s) 2 Au(s) + 3 Zn2+(aq)
Typed Answer 2Au3+(aq) + 3Zn(s) > 2Au(s) + 3Zn2+(aq)
(a) Write the half-cell reaction for the oxidation.
(b) Write the half-cell reaction for the reduction.
(c) Write the balanced equation for the cell reaction. Keep substances in the order given in the original equation.
(d) What are the following standard voltages? Include the sign. Use the standard reduction potentials in these Reference Tables. Enter the number of decimal places allowed by the data in the table.
oxidation half-cell
reduction half-cell
entire cell
(e) Select all that apply.
Ag1+ is the substance being oxidized.
Cu is the substance being oxidized.
Ag1+ is the substance being reduced.
Cu is the substance being reduced.
The forward reaction is spontaneous.
The reverse reaction is spontaneous.
Electrons will flow from the Ag half-cell to the Cu half-cell.
Electrons will flow from the Cu half-cell to the Ag half-cell.
[Ag1+] increases as the cell operates.
[Ag1+] decreases as the cell operates.
[Cu2+] increases as the cell operates.
[Cu2+] decreases as the cell operates.
[Ag1+] and [Cu2+] remain constant.
Ag1+ (aq) + Cu (s) Ag (s) + Cu2+ (aq)
Type the following answers using the formats given. Use only the format '1+' or '1-' for the charge on an ion. If only one electron is present in the half-cell reaction, type the answer as e- instead of 1e-.
Half-cell Equation Au3+(aq) + 3 e- Au(s)
Typed Answer Au3+(aq) + 3e- > Au(s)
Balanced Equation 2 Au3+(aq) + 3 Zn(s) 2 Au(s) + 3 Zn2+(aq)
Typed Answer 2Au3+(aq) + 3Zn(s) > 2Au(s) + 3Zn2+(aq)
(a) Write the half-cell reaction for the oxidation.
(b) Write the half-cell reaction for the reduction.
(c) Write the balanced equation for the cell reaction. Keep substances in the order given in the original equation.
(d) What are the following standard voltages? Include the sign. Use the standard reduction potentials in these Reference Tables. Enter the number of decimal places allowed by the data in the table.
oxidation half-cell
reduction half-cell
entire cell
(e) Select all that apply.
Ag1+ is the substance being oxidized.
Cu is the substance being oxidized.
Ag1+ is the substance being reduced.
Cu is the substance being reduced.
The forward reaction is spontaneous.
The reverse reaction is spontaneous.
Electrons will flow from the Ag half-cell to the Cu half-cell.
Electrons will flow from the Cu half-cell to the Ag half-cell.
[Ag1+] increases as the cell operates.
[Ag1+] decreases as the cell operates.
[Cu2+] increases as the cell operates.
[Cu2+] decreases as the cell operates.
[Ag1+] and [Cu2+] remain constant.