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Consider the electrochemical cell described below: What is the cell potential (Ecell) for the voltaic cell...
Consider the electrochemical cell described below: What is the cell potential (Ecell) for the voltaic cell described below if the.
Ag(s) çAg2CrO4 (Sat. Aq. Soln) çç Ag+ (0.125 M) ç
Ag(s)
a. What is the concentration of [Ag+] in the anode of the cell
described above, if the Ksp of
Silver (I) chromate is 1.1 x 10-12 ?
b. What is the Ecell?
c. Draw an overall cell diagram for this cell. Remember to label the cathode, anode, and electron flow.
please answer all
Solutions
Amanda K answered 6 months agoRelated Solutions
What is the difference between an electrochemical cell and a voltaic cell? Is there any? If...
What is the difference between an electrochemical cell and a
voltaic cell? Is there any? If they are different how do each of
their electrons flow?
What is the calculated value of the cell potential at 298K for an electrochemical cell with...
What is the calculated value of the cell potential at 298K for an
electrochemical cell with the following reaction, when the
Hg2+ concentration is
6.28×10-4 M and the
Al3+ concentration is
1.43 M ?
3Hg2+(aq)
+
2Al(s)------>3Hg(l)
+
2Al3+(aq)
Answer: ____V
The cell reaction as written above is spontaneous for the
concentrations given: _______(true)(false)
What is the calculated value of the cell potential at 298K for an electrochemical cell with...
What is the calculated value of the cell potential at 298K for an
electrochemical cell with the following reaction, when the
Hg2+ concentration is
1.18 M and the Mn2+
concentration is 8.88×10-4 M ?
Hg2+(aq) +
Mn(s)------>Hg(l)
+ Mn2+(aq)
Answer: ___V
The cell reaction as written above is spontaneous for the
concentrations given: _______(true)(false)
What is the calculated value of the cell potential at 298K for an electrochemical cell with...
What is the calculated value of the cell potential at 298K for
an electrochemical cell with the following reaction, when the Ag+
concentration is 1.49 M and the Al3+ concentration is 3.15×10-4 M ?
3Ag+(aq) + Al(s)3Ag(s) + Al3+(aq)
Answer: in V
The cell reaction as written above is spontaneous for the
concentrations given: True or False
What is the calculated value of the cell potential at 298K for
an electrochemical cell with the following reaction, when the Ag+
concentration...
If the cell potential for a voltaic cell is 0.250 V, and the reduction potential for...
If the cell potential for a voltaic cell is 0.250 V, and the
reduction potential for the oxidation reaction is ⎯0.150 V, what is
the reduction potential for the reaction occurring at the
cathode?
What is the standard cell potential, E°cell, for the spontaneous voltaic cell made by coupling a...
What is the standard cell potential, E°cell, for the
spontaneous voltaic cell made by coupling a Ca+2|Ca
(E°red=-2.756V) half-cell and a Al+3|Al
(E°red=-1.662V) half-cell? Report your answer in volts,
V.
Please show where you get the numbers, and write clearly please
:)
A voltaic cell consists of an Al/Al3+ half-cell and a Cd/Cd2+ half-cell. Calculate Ecell when [Cd2+]...
A voltaic cell consists of an Al/Al3+ half-cell and a Cd/Cd2+
half-cell. Calculate Ecell when [Cd2+] = 0.00303 M and [Al3+] =
0.47 M. You should use the reduction potentials for Al3+ is -1.66 V
and for Cd2+ is -0.40 V.
Determine the standard cell potential and the cell potential under the stated conditions for the electrochemical...
Determine the standard cell potential and the cell potential
under the stated conditions for the electrochemical
reactions described here. State whether each is spontaneous or
nonspontaneous under each set of conditions at
298.15 K.
(a) Hg(l) + S2-(aq, 0.10 M) + 2Ag+(aq, 0.25 M) ⟶ 2Ag(s) +
HgS(s)
(b) The galvanic cell made from a half-cell consisting of an
aluminum electrode in 0.015 M aluminum nitrate
solution and a half-cell consisting of a nickel electrode in 0.25 M
nickel(II) nitrate...
The cell potential of a redox reaction occurring in an electrochemical cell under any set of...
The cell potential of a redox reaction occurring in an
electrochemical cell under any set of temperature and concentration
conditions can be determined from the standard cell potential of
the cell using the Nernst equation E = E° − RT nF ln Q where E is
the cell potential of the cell, E° is the standard cell potential
of the cell, R is the gas constant, T is the temperature in kelvin,
n is the moles of electrons transferred in...
When [Ag+] = 1.05 M, the observed cell potential at 298K for an electrochemical cell with...
When [Ag+] = 1.05 M, the observed cell potential at 298K for an
electrochemical cell with the reaction shown below is 3.268 V. What
is the Mg2+ concentration in this cell?
2Ag+(aq) + Mg(s)-->2Ag(s) + Mg2+(aq)
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