|AP Chemistry - Electrochemistry Worksheet #6|
cell consists of a chromium electrode in a 1.0 mol/L solution of Cr(NO3)3,
a silver electrode in a 1.0 mol/L solution of AgNO3 and a salt
The spontaneous cell reaction is:
Cr(s) + 3 Ag+(aq) ---> Cr3+(aq) + 3 Ag(s)
If a 2.0 mol/L solution of NaCl is added to the beaker containing
|2.||The cell reaction
during the discharge of a lead storage battery is.
Pb(s) + PbO2(s) + 4 H1+(aq) + 2 SO42-(aq) --> 2 PbSO4(s) + 2 H2O
The standard cell potential is 2.05 V. What is the correct
form of the Nernst equation for this reaction?
|3.||The cell reaction
NiO2(s) + 4 H+(aq) + 2 Ag(s) ---> Ni2+(aq) + 2 H2O + 2 Ag+(aq)
has Eocell = 2.48 V. What will be
the cell potential at a pH of 6.00 when the concentrations of Ni2+
and Ag+ are each 0.10 M?
= 0.135 V for the reaction
3 I2(s) + 5 Cr2O72-(aq) + 34 H+(aq) -----> 6 IO3-(aq) + 10 Cr3+(aq) + 17 H2O
What is Ecell if [Cr2O72-]
= 0.10 M, [H1+] = 0.010 M,
|5.||A cell was set
up having the following reaction.
Mg(s) + Cd2+(aq) ----> Mg2+(aq) + Cd(s) Eocell = 1.97 V
The magnesium electrode was dipping into a 1.00 M solution of
MgSO4 and the cadmium was dipping into a solution of unknown
Cd2+ concentration. The potential of the cell was
measured to be 1.67 V. What was the unknown Cd2+ concentration?
|6.||A galvanic cell
was set up having the following half-reactions.
+ 2 e- ---> Fe(s) EoFe2+
= -0.440 V
The copper half-cell contained 100 mL of 1.00 M CuSO4.
The iron half-cell contained 50.0 mL of 0.100 M FeSO4. To the
iron half-cell was added 50.0 mL of 0.500 M NaOH solution. The mixture was
stirred and the cell potential was measured to be 1.175 V. Calculate
the value of Ksp for Fe(OH)2.
|7.||A cell employs
the following half-reactions.
+ 2 e- ---> Ni(s) EoNi2+
= -0.25 V
Calculate the potential if [Ni2+] = 1.0 x 10-4
and [Cr3+] = 2.0 x 10-3 M.
|8.||In a certain
Zn(s) + Cu2+(aq) ---> Zn2+(aq) + Cu(s)
The ion concentrations are [Cu2+] = 0.0100 M and
[Zn2+] = 1.0 M. What is the cell potential? The standard
potential is 1.10 V.
|9.||A galvanic cell
was constructed by connecting a nickel electrode that was dipping into 1.20
M NiSO4 solution to a chromium electrode that was dipping into
a solution containing Cr3+ at an unknown concentration.
The potential of the cell was measured to be 0.55 V, with the chromium serving
as the anode. What was the concentration of Cr3+ in
the solution of unknown concentration?
a galvanic cell were set up having the net cell reaction
Zn(s) + 2 Ag1+(aq) ---> Zn2+(aq) + 2 Ag(s)
The Ag1+ and Zn2+ concentrations in their respective half cells initially are 1.00 M, and each half-cell contains 100 mL of electrolyte solution. If this cell delivers current at a constant rate of 0.10 A, what will the cell potential be after 10.00 hr?