A.
A standard galvanic cell is constructed with
Cr3+|Cr and
Ag+|Ag half cell
compartments connected by a salt bridge. Which of the following
statements are correct?
Hint: Refer to a table of standard reduction potentials.
(Choose all that apply.)
1.As the cell runs, anions will migrate from the
Cr3+|Cr compartment to the Ag+|Ag
compartment.
2.The anode compartment is the Ag+|Ag
compartment.
3.Ag is oxidized at the anode.
4.Cr is oxidized at the anode.
5.In the external circuit, electrons flow from...
Write the half reaction for the anode and cathode for the
following electrochemical cells. which metal acts as the anode and
which acts as the cathode. For each cell, combine the half
reactions and write the overall cell reaction.
a. Zn/Cu
b. Fe/Cu
c. Mg/Cu
d. Pb/Cu
e. Sn/Cu
Write the half reaction for the anode and cathode for the
following electrochemical cells. which metal acts as the anode and
which acts as the cathode. For each cell, combine the half
reactions and write the overall cell reaction.
a. Zn/Cu
b. Fe/Cu
c. Mg/Cu
d. Pb/Cu
e. Sn/Cu
23. A voltaic cell is constructed with Cr3+/Cr and Zn2+/Zn
half-cells at 25 °C.
a. If the concentration of Zn2+ is 0.10 M, what concentration of
Cr3+ should be used so that the overall cell potential is 0 V?
b. What concentration of Cr3+ should you use to make the cell
consume Zn (s)?
c. What concentration of Cr3+ should you use to make the cell
deposit Zn (s)?
Write equations for the half-reactions that occur at the anode
and cathode for the electrolysis of each of the following aqueous
solutions. a) Ni(NO3)2 (aq) b)KCl (aq) c)CuBr2 (aq)
Take into account the aqueous solution. The oxidation and
reduction of water have to be considered for each
Write equations for the half-reactions that occur at the anode
and cathode for the electrolysis of each of the following aqueous
solutions.
Part A Ni(NO3)2(aq) Express your answers as chemical equations
separated by a comma. Identify all of the phases in your
answer.
Part B KCl(aq) Express your answers as chemical equations
separated by a comma. Identify all of the phases in your
answer.
Part C CuBr2(aq) Express your answers as chemical equations
separated by a comma. Identify all of...
For the following electrochemical cell
Cu(s)|Cu^2+ (aq, 0.0155
M)||Ag^+ (aq, 3.50 M)|Ag(s)
write the net cell equation. Phases are optional. Do not include
the concentrations.
Calculate the following values at 25.0 °C using standard
potentials as needed.
Eocell
delta Go reaction
Ecell
delta G reaction
Copper can be electroplated at the cathode of an electrolysis
cell by the half-reaction.
Cu2+(aq)+2e−→Cu(s)Cu2+(aq)+2e−→Cu(s)
Part A
How much time would it take for 338 mgmg of copper to be plated
at a current of 7.1 AA ?
A voltaic cell consists of a Zn/Zn2+ anode and a
Ni/Ni2+ cathode at 25 ∘C. The initial
concentrations of Ni2+ and Zn2+ are 1.7 M and
0.12 M , respectively. The volume of half-cells is the same.
What is the concentration of Ni2+ when the cell
potential falls to 0.456 V ?
Enter your answer to 4 decimal places and in units of mM.
Zn2+ (aq) + 2 e- ⟶Zn(s) E° = -0.76 V
Ni2+ (aq) + 2 e- ⟶ ...