Question
In: Chemistry
a) Calculate the potential in the following cell (no current is flowing) Zn|Zn2+(1.00M)|| UO2 2+(1.00M), U4+...
a) Calculate the potential in the following cell (no current is flowing)
Zn|Zn2+(1.00M)|| UO2 2+(1.00M), U4+ (0.1M), H3O + (1.00M) |Pt
b) The cathode has a volume of 50 mL. What is the cell potential (no current) after adding 10 mL, 25 mL, 50 mL, and 100 mL 1M NaOH to the cathode?
c) What is the Gibbs Free Energy for the 5 cells in a) and b). What is the spontaneous reaction in each case?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
a) Calculate the potential in the following cell (no current is flowing) Zn|Zn2+(1.00M)|| UO2 2+(1.00M), U4+...
a) Calculate the potential in the following cell (no current is
flowing)
Zn|Zn2+(1.00M)|| UO2 2+(1.00M),
U4+ (0.1M), H3O + (1.00M) |Pt
b) The cathode has a volume of 50 mL. What is the cell potential
(no current) after adding 10 mL, 25 mL, 50 mL, and 100 mL 1M NaOH
to the cathode?
c) What is the Gibbs Free Energy for the 5 cells in a) and b).
What is the spontaneous reaction in each case?
Zn|Zn2+(1.00M)|| UO22+(1.00M), U4+(0.1M), H3O+(1.00M) |Pt a) Calculate the potential in the following cell (no current is...
Zn|Zn2+(1.00M)|| UO22+(1.00M), U4+(0.1M), H3O+(1.00M) |Pt
a) Calculate the potential in the following cell (no current is
flowing)
b) The cathode has a volume of 50 mL. What is the cell potential
(no current) after adding 10 mL, 25 mL, 50 mL, and 100 mL 1M NaOH
to the cathode?
c) What is the Gibbs Free Energy for the 5 cells in a) and b).
What is the spontaneous reaction in each case?
Calculate the cell potential for the following electrochemical cell: Zn | [Zn2+]=4.2M || [Cu2+]=0.004M | Cu
Calculate the cell potential for the following electrochemical cell:
Zn | [Zn2+]=4.2M || [Cu2+]=0.004M | Cu
Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Zn2...
Calculate the cell potential for the following reaction as
written at 25.00 °C, given that [Zn2 ] = 0.763 M and [Sn2 ] =
0.0140 M. Standard reduction potentials can be found here.
Zn(s)+SN2+ YIELDS Zn2+(aq)+Sn(s)
The standard cell potential, E°, for Br2(aq) + Zn(s) → 2Br-(aq) + Zn2+(aq) at 298K is...
The standard cell potential, E°, for Br2(aq) + Zn(s)
→ 2Br-(aq) + Zn2+(aq) at 298K is 1.82V.
Calculate the value of ΔG° in kJ. Use 96,485 C/mol e-.
Then calculate the equilibrium constant for the data.
For a concentration cell: Zn/Zn2+ (0.05M)//Zn2+(1M)/Zn E= 0.035 volt a. What can you say about the...
For a concentration cell:
Zn/Zn2+ (0.05M)//Zn2+(1M)/Zn
E= 0.035 volt
a. What can you say about the measured emf of this cell and the
concentration cell of Cu/Cu2+ (0.05M)//Cu2+(1M)/Cu ?
b. Why is the standard emf (E) not a factor in these two
cells?
c. Use the Nernst equation to calculate the emf of this
cell.
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ∘C. The...
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
1.30mol/L and 0.130 mol/L, respectively.
Zn2+(aq)+2e−→Zn(s)E∘=−0.76V
Ni2+(aq)+2e−→Ni(s)E∘=−0.23V
What are the concentrations of Ni2+ and Zn2+ when the cell
potential falls to 0.45 V?
Express your answers using two significant figures separated by
a comma.
A voltaic cell consists of a Zn/Zn2+ half-cell and a Ni/Ni2+ half-cell at 25 ∘C. The...
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
1.50 M and 0.110 M , respectively. The volume of half-cells is the
same.
Part A
What is the initial cell potential?
Part B
What is the cell potential when the concentration of Ni2+ has
fallen to 0.600 M ?
Part C
What is the concentrations of Ni2+ when the cell potential falls
to 0.46 V ?...
The voltage generated by the zinc concentration cell described by, Zn(s)|Zn2 (aq, 0.100 M)||Zn2 (aq, ?...
The voltage generated by the zinc concentration cell described
by,
Zn(s)|Zn2 (aq, 0.100 M)||Zn2 (aq, ? M)|Zn(s)
is 26.0 mV at 25 °C. Calculate the concentration of the Zn2 (aq)
ion at the cathode.
A voltaic cell consists of a Zn/Zn2+ anode and a Ni/Ni2+ cathode at 25 ∘C. The...
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- ⟶ ...
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