Question

Consider the Daniell cell, for which the overall cell reaction is Zn(s)+Cu2+(aq)⇌Zn2+(aq)+Cu(s) The concentrations of CuSO4 and ZnSO4 are 2.20×10−3 m and 1.10×10−3 m , respectively.

Part A

Calculate E setting the activities of the ionic species equal to
their molalities.

Express your answer to four significant figures and include the
appropriate units.

E = ?

Part B

Calculate γ±,ZnSO4 for the half-cell solutions using the
Debye-Huckel limiting law.

Express your answer using three significant figures.

γ±,ZnSO4 = ?

Part C

Calculate γ±,CuSO4 for the half-cell solutions using the
Debye-Huckel limiting law.

Express your answer using three significant figures.

γ±,CuSO4 = ?

Part D

Calculate E using the mean ionic activity coefficients
determined in part (b) and part (c).

Express your answer to four significant figures and include the
appropriate units.

E = ?

Answer #1

A voltaic cell is constructed that uses the following reaction
and operates at 298 K:
Zn(s)+Ni2+(aq)→Zn2+(aq)+Ni(s).
A)
What is the emf of this cell when [Ni2+]= 3.70 M and [Zn2+]=
0.100 M ?
Express your answer using two significant figures.
B)
What is the emf of the cell when [Ni2+]= 0.270 M and [Zn2+]=
0.860 M ?
Express your answer using two significant figures.

A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+
half-cell at 25 ∘C. The initial concentrations of Ni2+ and Zn2+ are
1.80 M and 0.130 M , respectively. The volume of half-cells is the
same.
a) What is the initial cell potential?
Express your answer using two significant figures.
b) What is the cell potential when the concentration of Ni2+ has
fallen to 0.600 M ?
Express your answer using two significant figures.

1)
A Cu/Cu2+ concentration cell has
a voltage of 0.21 V at 25 ∘C. The concentration of Cu2+ in one of
the half-cells is 1.5×10−3 M .
What is the concentration of Cu2+ in the other half-cell?
Express your answer using two significant figures.
2)
Galvanized nails are iron nails that have been plated with zinc
to prevent rusting. The relevant reaction is
Zn2+(aq)+2e−→Zn(s)
For a large batch of nails, a manufacturer needs to plate a
total zinc mass of...

Consider the reaction
Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)
at 79 ∘C , where [Fe2+]= 3.30 M and [Mg2+]= 0.310
M .
Part A
What is the value for the reaction quotient, Q, for the
cell?
Part B
What is the value for the temperature, T, in
kelvins?
Express your answer to three significant figures and include the
appropriate units.
Part C
What is the value for n?
Express your answer as an integer and include the appropriate
units (i.e. enter mol for moles).
Part...

A)
A galvanic cell
Zn(s)|Zn2+(aq) ||
Ni2+(aq)|Ni(s) is
constructed using a completely immersed Zn
electrode that weighs 43.2 g and a
Ni electrode immersed in 503 mL
of 1.00 M Ni2+(aq) solution. A steady
current of 0.0555 A is drawn from the cell as the
electrons move from the Zn electrode to the
Ni electrode.
Which reactant is the limiting
reactant in this cell?
Enter symbol
___________
How long does it take for the cell to be completely discharged?
_____s...

Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 69 ∘C ,
where [Fe2+]= 3.20 M and [Mg2+]= 0.110 M .
Part A:What is the value for the reaction quotient, Q,
for the cell?
Express your answer numerically.
Part B:What is the value for the temperature, T, in
kelvins?
Express your answer to three significant figures and
include the appropriate units.
Part C:What is the value for n?
Express your answer as an integer and include the
appropriate units (i.e. enter mol for moles)....

1.A Cu/Cu2+ concentration cell (E∘=0.34V) has a voltage
of 0.24 V at 25 ∘C. The concentration of Cu2+ in the cathode is
1.4×10−3 molL−1.
What is the concentration of Cu2+ in anode?
Express your answer using two significant figures.
2. The following reaction is spontaneous as written when the
components are in their standard states:
3 Zn(s) +2 Cr3+(aq) →3
Zn2+(aq) +2 Cr(s)
If the [Zn2+] is 3 molL−1, determine the value of [Cr3+] below
which the reaction will be...

Given the cell reaction : 2 Cl – (aq) + Cu2+(aq)→ Cl2 (aq) + Cu
(s)
a) As written, is the cell galvanic or electrolytic?
b) Calculate E°cell.
c) Calculate ΔG°.
3. Using the standard reduction potentials given in Appendix of
your text book, calculate the cell potential (E°cell ) at 298 K for
each of the following reactions.
(A) Br2 (aq) + 2 ClV (aq) → 2BrV (aq) + Cl2 (g)
(B) A Galvanic Cell with the SHE and...

Use the standard reduction potentials shown here to answer the
questions.
Reduction half-reaction
E∘ (V)
Cu2+(aq)+2e−→Cu(s)
0.337
2H+(aq)+2e−→H2(g)
0.000
A copper, Cu(s), electrode is immersed in a solution that is
1.00 M in ammonia, NH3, and 1.00 M in
tetraamminecopper(II), [Cu(NH3)4]2+. If a standard hydrogen
electrode is used as the cathode, the cell potential,
Ecell, is found to be 0.073 V at 298 K.
Part A
Based on the cell potential, what is the concentration of Cu2+
in this solution?...

Calculate the standard cell potential for each of the
electrochemical cells. Part A 2Ag+(aq)+Pb(s)?2Ag(s)+Pb2+(aq)
Express your answer using two significant figures. Part B
2ClO2(g)+2I?(aq)?2ClO?2(aq)+I2(s) Express your answer using two
significant figures. Part C
O2(g)+4H+(aq)+2Zn(s)?2H2O(l)+2Zn2+(aq)

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