Question

A voltaic (galvanic) cell is constructed using a manganese
electrode placed in 1.00 L of a 0.272 *M* MnSO_{4}
solution and a nickel electrode placed in 1.00 L of a 0.0146
*M* NiSO_{4} solution at 25°C. Determine the
starting cell potential in (V).

Answer #1

A voltaic cell is constructed by connecting a nickel electrode
that is dipped into 1.20 M NiSO4 solution to a chromium electrode
that is dipped into a solution containing Cr3+ at an unknown
concentration. The potential of the cell is measured to be 0.552 V.
What is the concentration of the Cr3+ in the solution?
5.3 x 10‒3 M
9.5 x 10‒4 M
1.3 x 10‒5 M
2.9 x 10‒4 M
5.8 x 10‒5 M

A galvanic cell is constructed with a silver-silver chloride
electrode, and a nickel strip immersed in a beaker containing 5.56
x 10-2 M solution of NiC12. Determine the balanced cell reaction
and calculate the potential of the cell. Enter in volts. (assume a
temperature of 25°C) The answer is not .97

A galvanic (voltaic) cell consists of an electrode composed of
magnesium in a 1.0 M magnesium ion solution and another electrode
composed of gold in a 1.0 M gold(III) ion solution, connected by a
salt bridge. Calculate the standard potential for this cell at 25
°C. Standard reduction potentials can be found here.

A voltaic cell contains two half-cells. One half-cell contains a
nickel electrode immersed in a 1.00 M
Ni(NO3)2 solution. The second half-cell
contains a titanium electrode immersed in a 1.00
MTi(NO3)3 solution.
Ni2+(aq) + 2 e− →
Ni(s)
E⁰red = −0.257 V
Ti3+(aq) + 3 e− →
Ti(s)
E⁰red = −1.370 V
(a) Using the standard reduction potentials given above, predict
the standard cell potential of the voltaic cell.
____V
(b) Write the overall balanced equation for the voltaic cell....

A galvanic (voltaic) cell consists of an electrode composed of
iron in a 1.0 M iron(II) ion solution and another electrode
composed of silver in a 1.0 M silver ion solution, connected by a
salt bridge. Calculate the standard potential for this cell at 25
°C. Standard reduction potentials can be found here
(https://sites.google.com/site/chempendix/potentials)

A voltaic cell is constructed in which the cathode is a standard
hydrogen electrode and the anode is a hydrogen electrode
(P(H2) = 1 atm) immersed in a solution of unknown
[H+]. If the cell potential is 0.179 V,
what is the pH of the unknown solution at 298 K?

A galvanic cell consists of a zinc electrode in 0.0514 M
Zn(NO3)2 and a nickel electrode in 0.379 M
Ni(NO3)2. What is the cell potential (emf, in
V) of this cell at 25oC?

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...

A galvanic cell consists of an electrode of Pb in a 0.03 M
solution of PbSO4 and an electrode of Sn in a solution of 0.7 M
SnSO4 at 25°C. What is the emf of the cell?

The line notation for the galvanic cell is:
Ni | NiSO4 (aq) || CuCl2 (aq) | Cu
a) write reduction half-reactions for each electrode.
b) what is the standard potential for the cell?
c) what is the equilibrium constant for the cell?
d) if the cell delivers a constant current of 19.0mA for 6.00
hours, how many grams of nickel will be consumed?

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