Question

For the following electrochemical cells, calculate the potential and determine if the cell reaction is spontaneous as written at 25°C.

Pt(s) ΙSn2 (0.0055 M), Sn4 (0.12 M) ΙΙFe2 (0.0020 M), Fe3 (0.15 M) ΙPt(s)

Ecell=? V

Answer #1

A) What is the calculated value of the cell potential at 298K
for an electrochemical cell with the following reaction, when the
Cl2 pressure is
8.15×10-4 atm, the
Cl- concentration is
1.48M, and the Pb2+
concentration is 1.07M ?
Cl2(g) +
Pb(s) --->
2Cl-(aq)
+ Pb2+(aq)
Answer: _____ V
The cell reaction as written above is spontaneous for the
concentrations given:____ ( TRUE/FALSE )
B)What is the calculated value of the cell potential at 298K for
an electrochemical cell with...

What is the cell potential for the spontaneous concentration
cell with the reaction Fe3+(aq) + Fe(s) → Fe(s) + Fe3+(aq), with
concentrations of Fe3+ of 0.873M and 0.342M at a temperature of
310. K? Ecell = E°cell −(RT/nF)lnQ

Please show work
Calculate the cell potential for the following reaction that
takes place in an electrochemical cell at 25°C. Mn(s) ∣ Mn2+(aq,
1.28 M) ∥ Ag+(aq, 0.000837 M) ∣ Ag(s) Calculate the cell potential
for the following reaction that takes place in an electrochemical
cell at 25°C. Mn(s) Mn2+(aq, 1.28 M) Ag+(aq, 0.000837 M) Ag(s)
1.98 V
0.00 V
1.79 V
-0.84 V
-1.28 V

What is the calculated value of the cell potential at 298K for
an electrochemical cell with the following reaction, when the Cu2+
concentration is 1.23 M and the Cr3+ concentration is 5.82×10-4 M ?
3Cu2+(aq) + 2Cr(s)-->3Cu(s) + 2Cr3+(aq) Answer: V The cell
reaction as written above is spontaneous for the concentrations
given

What is the calculated value of the cell potential at 298K for
an electrochemical cell with the following reaction, when the Cu2+
concentration is 7.38×10-4 M and the Al3+ concentration is 1.43 M
?
3Cu2+(aq) + 2Al(s)3Cu(s) + 2Al3+(aq)
Answer: V
The cell reaction as written above is spontaneous for the
concentrations given: True or False?

What is the calculated value of the cell potential at 298K for
an electrochemical cell with the following reaction, when the Pb2+
concentration is 1.20 M and the Mn2+ concentration is 5.43×10-4 M
?
Pb2+(aq) + Mn(s) Pb(s) + Mn2+(aq)
Answer: in V
The cell reaction as written above is spontaneous for the
concentrations given: true or false?

What is the calculated value of the cell potential at 298K for
an electrochemical cell with the following reaction, when the Cu2+
concentration is 1.44 M and the Mg2+ concentration is 1.47×10-4 M
?
Cu2+(aq) + Mg(s) Cu(s) + Mg2+(aq)
Answer: V
The cell reaction as written above is spontaneous for the
concentrations given:
_______
true
false

The cell potential of the following electrochemical cell depends
on the pH of the solution in the anode half-cell:
Pt(s)|H2(g,1atm)|H+(aq,?M)||Cu2+(aq,1.0M)|Cu(s). What is the pH of
the solution if Ecell is 360 mV ?

What is the calculated value of the cell potential at 298 K for
an electrochemical cell with the following reaction, when the
H2 pressure is
5.00×10-3 bar, the
H+ concentration is
1.46 M, and the
Zn2+concentration is
3.42×10-4 M ?
2H+(aq)
+ Zn(s) ---->
H2(g) +
Zn2+(aq)
Answer: _____ V ?
The cell reaction as written above is product-favored (spontaneous)
for the concentrations given: _______(true/false)?

Calculate the theoretical potential of the following cell. Is
this cell as written galvanic or electrolytic? Pt | Cr3+ (3.00x10-2
M), Cr2+ (4.00x10-5 M) || Sn2+ (2.00x10-2 M), Sn4+ (2.00x10-4 M)|
Pt

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