Question
In: Chemistry
Consider a concentration cell. Two Ag-electrodes are immersed in AgNO3 solutions of different concentrations. When the...
Consider a concentration cell. Two Ag-electrodes are immersed in
AgNO3 solutions of different concentrations. When the two
compartments have an AgNO3-concentration of 1 M and 0.1 M,
respectively, the measured voltage is 0.065 V (note: T in not
necessarily = 25°C !).
a. What is the voltage, if the two compartments have AgNO3-concentration of 1 M and 0.01 M, respectively?
The electrochemical behavior of silver nanoclusters (Agn, with n
the number of Ag atoms in the cluster) is investigated using the
following electrochemical cells at 298 K:
I. Ag(s) | AgCl (saturated) || Ag+(aq, 0.01M) |
Ag(s), E=0.170
II. (Pt electrode) Agn (s, nanocluster) | Ag+(aq,
0.01M) || AgCl (saturated) | Ag(s), with E = +1.030 V for
Ag5 nanocluster and E = +0.430 V for Ag10 nanocluster
The standard reduction potential for Ag+ + e- → Ag, is E0 = +0.800 V.
b. Use this data to calculate the solubility product of AgCl.
The two nanoclusters Ag5 and Ag10-nanoclusters have standard potentials different from the potential of metallic bulk silver.
c. Calculate the standard potentials of Ag5 and of Ag10 nanoclusters. [for this part use Ksp(AgCl)=1.800·10-5; this is not the same value as calculated in b.]
d. What happens, if you put the Ag10 nanoclusters and – in a second experiment – the Ag5 nanoclusters into an aqueous solution of pH=5? Estimate the consequences using the reduction potentials you calculated.
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
-- Consider a concentration cell. Two Ag-electrodes are immersed in AgNO3 solutions of different concentrations. When...
-- Consider a concentration cell. Two Ag-electrodes are immersed
in AgNO3 solutions of different concentrations. When the two
compartments have an AgNO3-concentration of 1 M and 0.1 M,
respectively, the measured voltage is 0.065 V (note: T in not
necessarily = 25°C ).
The electrochemical behavior of silver nanoclusters (Agn, with n
the number of Ag atoms in the cluster) is investigated using the
following electrochemical cells at 298 K:
I. Ag(s) | AgCl (saturated) || Ag+(aq, 0.01M)
| Ag(s),...
The solutions at the two Pb electrodes of a concentration cell were prepared as follows: Cell...
The solutions at the two Pb electrodes of a concentration cell
were prepared as follows:
Cell A: A mixture of 1.00 mL of 0.0500 M
Pb(NO3)2 with 4.00 mL of 0.0500 M KX (the
soluble potassium salt of an unspecified monovalent ion
X-).
Some PbX2(s) precipitates.
Cell B: 5.00 mL of 0.0500 M Pb(NO3)2.
The cell potential was measured to be 0.05600 V at 25 °C.
1.By use of the Nernst equation, determine the concentration (M)
of Pb2+ in the...
The solutions at the two Pb electrodes of a concentration cell were prepared as follows: Cell...
The solutions at the two Pb electrodes of a concentration cell
were prepared as follows:
Cell A: A mixture of 1.00 mL of 0.0500 M
Pb(NO3)2 with 4.00 mL of 0.0500 M KX (the soluble potassium salt of
an unspecified monovalent ion X-). Some PbX2(s) precipitates.
Cell B: 5.00 mL of 0.0500 M Pb(NO3)2.
The cell potential was measured to be 0.05100 V at 25 °C.
1.)By use of the Nernst equation, determine the concentration
(M) of Pb2+ in the...
An electrochemical cell is composed of pure copper and pure lead electrodes immersed in solutions of...
An electrochemical cell is composed of pure copper and pure lead
electrodes immersed in solutions of their respective divalent ions.
For a 0.7 M concentration of Cu2+, the lead
electrode is oxidized yielding a cell potential of 0.520 V.
Calculate the concentration of Pb2+ ions if the
temperature is 25˚C. The standard potentials for Cu and Pb are
+0.340 V and -0.126 V.
Please show your work!
A rechargeable battery is constructed based on a concentration cell constructed of two Ag/Ag+ half-cells. The...
A rechargeable battery is constructed based on a concentration
cell constructed of two Ag/Ag+ half-cells. The volume of each
half-cell is 1.9 L and the concentrations of Ag+ in the half-cells
are 1.20 M and 1.2×10−3M.
Part A
How long can this battery deliver 2.7 A current before it
dies?
Express your answer using two significant figures.
A rechargeable battery is constructed based on a concentration cell constructed of two Ag/Ag+ half-cells. The...
A rechargeable battery is constructed based on a concentration
cell constructed of two Ag/Ag+ half-cells. The volume of each
half-cell is 1.8 L and the concentrations of Ag+ in the half-cells
are 1.35 M and 1.0×10−3 M .
a) For how long can this battery deliver 2.8 A of current before
it goes dead?
b) What mass of silver is plated onto the cathode by running at
3.8 A for 5.7 h ?
c) Upon recharging, how long would it...
A rechargeable battery is constructed based on a concentration cell constructed of two Ag/Ag+ half-cells. The...
A rechargeable battery is constructed based on a concentration
cell constructed of two Ag/Ag+ half-cells. The volume of each
half-cell is 2.2 L and the concentrations of Ag+ in the half-cells
are 1.25 M and 1.2×10−3 M .
At which half-cell does the concentration of Ag+ decrease as the
cell is run? What is the initial concentration of Ag+ at that
half-cell?
At which half-cell does the concentration of Ag+
decrease as the cell is run?
What is the initial...
Osmosis occurs when two solutions of different concentrations are separated by a semipermeable membrane. The membrane...
Osmosis occurs when two solutions of different concentrations
are separated by a semipermeable membrane. The membrane allows
solvent particles, but not solute particles, to pass through. Thus,
the solvent moves toward the solution of higher concentration (to
dilute it) until the two solutions have the same concentration, or
until gravity overtakes the osmotic pressure, Π. The osmotic
pressure between a solution and pure solvent depends on the number
of solute particles and thus is a colligative property. It can be...
When the Ag+ concentration is 1.31 M, the observed cell potential at 298K for an electrochemical...
When the Ag+ concentration is
1.31 M, the observed cell potential at 298K for an
electrochemical cell with the following reaction is
1.672V. What is the
Zn2+ concentration?
2Ag+(aq)
+
Zn(s)---->2Ag(s)
+ Zn2+(aq)
Answer: _______M
1) When the Ag+ concentration is 1.08 M, the observed cell potential at 298K for an...
1) When the Ag+ concentration is
1.08 M, the observed cell potential at 298K for an
electrochemical cell with the following reaction is
1.654V. What is the
Zn2+ concentration?
2Ag+(aq)
+ Zn(s) >
2Ag(s) +
Zn2+(aq)
Answer: ___ M
2) A concentration cell similar to the one shown is composed of
two Cr electrodes and solutions of different
Cr3+concentrations. The left
compartment contains 1.32 M
Cr3+, and the right compartment
contains 0.250 M
Cr3+.
Calculate the cell potential for this...
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