Question

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

Answer #1

**1) Ni(s) = Ni^2+(aq) + 2e^-**

**2) 2Ag^+(aq) + 2e^- = 2Ag(s)**

**E^o(cell) = E^o(cathode) - E^o(anode) = 0.80 V - (-0.23
V) = 0.80 V + 0.23 V = 1.03 V**

**Solve for [Ni^2+]:**

**Ratio of NiCl2:Ni^2+ is 1:1, so [Ni^2+] = 3.97 x 10^-2
M**

**Solve for [Ag^+]:**

**Ksp = [Ag^+] [Cl^-] ... let x = [Ag^+] =
[Cl^-]**

**(1.77 x 10^-10) = x^2 ... solve for x**

**x = square root (1.77 x 10^-10) = 1.33 x 10^-5
M**

**Solve for Q:**

**Q = [Ni^2+] / [Ag^+]^2 = (3.97 x 10^-2) / (1.33 x
10^-5)^2 = 2.24 x 10^8**

**Solve for E(cell):**

**E(cell) = E^o(cell) - (0.0592 / n) log Q**

**E(cell) = 1.03 - (0.0592 / 2 moles of e^-) log (2.24 x
10^8)**

**E(cell) = 0.783
V**

A voltaic (galvanic) cell is constructed using a manganese
electrode placed in 1.00 L of a 0.272 M MnSO4
solution and a nickel electrode placed in 1.00 L of a 0.0146
M NiSO4 solution at 25°C. Determine the
starting cell potential in (V).

A cell composed of a platinum indicator electrode and a
silver-silver chloride reference electrode in a solution containing
both Fe2 and Fe3 has a cell potential of 0.698 V. If the
silver-silver chloride electrode is replaced with a saturated
calomel electrode (SCE), what is the new cell potential?

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 voltaic cell was constructed by
placing a strip of silver in a solution of 1.0 M silver (I) acetate
and a strip of chromium in a solution of 1.0 M chromium (III)
nitrate. The two solutions were connected through a tube containing
a gel impregnated with KCl. (A) Write half reactions and identify
the cathode and the anode. (B) What is the electrical potential of
this cell?

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 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 galvanic cell consists of a silver electrode in 1 M AgNO3 and
a chromium electrode in 1 M Cr(NO3)3. What is the equilibrium
constant for this reaction at 25oC? Enter you answer with 2
significant digits, using the syntax of "1.0x10(22)" for
"1.0x1022"

Consider an electrochemical cell with a zinc electrode immersed
in 1.0 M Zn2+ and a nickel electrode immersed in 0.10 M Ni2+.
Calculate the concentration of Ni2+ if the cell is allowed to run
to equilibrium at 25 degrees C.

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)

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