Question

Given a potential of 0.456 V, for the following electrochemical cell, what is the concentration of Ag+?

Cu2+(aq) (1.0 M)|Cu(s)||Ag+(aq)|Ag(s)

Answer #1

The first that we need to define are the reactions involved, and by the nomenclature of the cell we can see that in the anode is taking place the oxidation of the Cu, and in the cathode the reduction of the Ag, if we look in a table of reduction potentials.

now, we need to turn around the equation of the Cu to obtain the oxidation reaction (remember that this will change the sign of the potential) and multiply the Ag reaction by 2, in order to obtain the global reaction of the cell.

if we evaluate the Nernst equation,

from this equation we already know the potential of the cell, E,
the estandar potencial, E^{0} , the numbers of moles of
electrons, n, and the concentration of Cu^{+2} , 1M. We
only need to isolate the Ag^{+} concentration.

The concentration of Ag^{+} is 0,855 M.

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

When the Cu2+ concentration is
1.40 M, the observed cell potential at 298K for an
electrochemical cell with the following reaction is
2.805V. What is the
Mg2+ concentration?
Cu2+(aq) +
Mg(s) ----->
Cu(s) +
Mg2+(aq)
Answer: ______M

A) When the Cu2+ concentration is
1.07 M, the observed cell potential at 298K for an
electrochemical cell with the following reaction is
1.607V. What is the
Mn2+ concentration?
Cu2+(aq) +
Mn(s)-->
Cu(s) +
Mn2+(aq)
Answer: _____ M
B) When the Cu2+ concentration is
5.71×10-4 M, the observed cell
potential at 298K for an electrochemical cell with the following
reaction is 2.609V. What is the
Mg2+ concentration?
Cu2+(aq) +
Mg(s)--->
Cu(s) +
Mg2+(aq)
Answer: _____ M
C) When the Cu2+...

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?

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 ?

Write the net cell
equation for the electrochemical cell. Phases are optional. Do not
include the concentrations.
Cu(s)∣∣Cu2+(aq,0.0155
M)∥∥Ag+(aq,3.50 M)∣∣Ag(s)Cu(s)|Cu2+(aq,0.0155 M)‖Ag+(aq,3.50
M)|Ag(s)
net cell equation:
Calculate E∘cellEcell° and EcellEcell at 25 °C25 °C, using
standard potentials as needed.

1. What is the calculated value of the cell potential at 298K
for an electrochemical cell with the following reaction, when the
Pb2+ concentration is
4.09×10-4 M and the
Mg2+ concentration is
1.03 M ?
Pb2+(aq) +
Mg(s) --->
Pb(s) +
Mg2+(aq)
Answer: ___V
The cell reaction as written above is spontaneous for the
concentrations given____. (true or false)
(From the table of standard reduction potentials: )
Pb2+(aq) + 2 e- --> Pb(s)
-0.126
Mg2+(aq) + 2 e- --> Mg(s)...

Electrochemical Cell Potentials
Table 1: Electrochemical
Cell Potentials
Cell
Measured Total Potential
from Multimeter (V)1
Individual Half-Cell
Potentials
Cell
Reactions5
ΔG
(kJ)6
(Cu) Electrode Standard
Potential (V)2
Metal Electrode
Experimental
Potential
(V)3
Metal Electrode
Theoretical
Potential
(V)4
Metal Electrode
Potential
% Error
Cu | Sn
0.469
0.34 V
0.34-0.469
=-0.129
Cathode:
Cu2+ + 2e- -> Cu
Anode:
Sn ->Sn2++ 2e-
Net:
Cu2+ + Sn -> Cu + Sn2+
Cu | Al
0.796
0.34 V
0.34-0.796
=-0.456
Cathode:
Cu2+ +...

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...

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