Question
In: Chemistry
Sketch and briefly explain a cell composed of 1 M CuSO4, Cu electrode and 1 M...
Sketch and briefly explain a cell composed of 1 M CuSO4, Cu electrode and 1 M ZnSO4 and a Zn electrode, Calculate the Emf and don’t forget to show the salt bridge.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
(a) The cell of interest in this figure is: Cu(s) | CuSO4(aq, 1.0 M) | KCl(aq,...
(a) The cell of interest in this figure is: Cu(s) | CuSO4(aq,
1.0 M) | KCl(aq, 3 M) | AgCl(s) | Ag(s) Write reduction
half-reactions for this cell. (Omit states-of-matter from your
answer.)
Calculate the ∆G for a cell composed of a Zn electrode in a 1.0 M Zn(NO3)3...
Calculate the ∆G for a cell composed of a Zn electrode in a 1.0
M Zn(NO3)3 solution and an Al electrode in a 0.1 M Al(NO3)3
solution at 298 K.
A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II)...
A galvanic (voltaic) cell consists of an electrode composed of
nickel in a 1.0 M nickel(II) 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.
____V
2)Consider these two entries from a fictional table of standard
reduction potentials.
X2+ + 2e- => X(s) E=2.26 V
Y2+ + 2e- => Y(s) E=0.14 V
Which pair of species would react under...
An electrochemical cell, composed of an iron electrode (anode) immersed in 0.10 M Fe (NO3)2 and...
An electrochemical cell, composed of an iron electrode (anode)
immersed in 0.10 M Fe (NO3)2 and silver electrode (cathode)
immersed in 0.11M AgNO3, was found to have a cell potential of
1.21V. The standard reduction potential for Ag+ / Ag half-cell is
+0.80V. The standard reduction potential for the Fe+2/ Fe half –
cell is -0.45V.
1. Write the half-cell reaction at the anode.
2.Write the half –cell reaction at the Cathode
3.Write over all cell
reaction
4. Determine the...
PART A: Calculate the ∆G for a cell composed of a Zn electrode in a 1.0...
PART A: Calculate the ∆G for a cell composed of
a Zn electrode in a 1.0 M Zn(NO3)3 solution and an Al electrode in
a 0.1 M Al(NO3)3 solution at 298 K.
PART B: Write the net ionic equation describing
the reaction occurring spontaneously in the cell described in PART
A.
PART C: Calculate the G for this cell at
298K.
Consider the voltaic cell composed of a Mn/Mn2+ electrode and a Fe/Fe2+ electrode. Calculate the concentration...
Consider the voltaic cell composed of a Mn/Mn2+ electrode and a
Fe/Fe2+ electrode. Calculate the concentration of Fe2+ if the
concentration of Mn2+ is 0.010 M and Ecell is 0.78V.
A galvanic cell consists of a iron electrode in 1 M Fe(NO3)2 and a copper electrode...
A galvanic cell consists of a iron electrode in 1 M Fe(NO3)2 and
a copper electrode in 1 M Cu(NO3)2. 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"
A galvanic cell consists of a iron electrode in 1 M Fe(NO3)2 and a copper electrode...
A galvanic cell consists of a iron electrode in 1 M Fe(NO3)2 and
a copper electrode in 1 M Cu(NO3)2. 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
What is the cell potential (emf, in V) of this cell at
25oC?
Cu |Cu2+ (0.0510 M) ‖ Br2 |Br-
(0.363 M)
What mass (in g) of aluminum can be electroplated when 0.855
amps are used...
The arrangement of using Mg/MgSO4 and Cu/CuSO4 couples as the half-cells to create a galvanic cell....
The arrangement of using Mg/MgSO4 and Cu/CuSO4 couples as the
half-cells to create a galvanic cell.
a) Draw a picture showing a Daniell cell-type experimental
apparatus using the half-cells stated in this problem.
b) Write the notation for a cell diagram for this galvanic
cell.
c) Identify the anode.
d) Identify the cathode.
e) Indicate the signs of the electrodes.
f) Describe the flow of electrons through the external wire.
g) Describe the flow of ions in the salt bridge.
A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3,...
A copper, Cu(s), electrode is immersed in a solution that is
1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II),
[Cu(NH3)4]^{2+}. If a standard hydrogen electrode is used as the
cathode, the cell potential, Ecell, is found to be 0.075 V at 298
K.
Half reaction of Cu = .337 V
Half reaction of H = .000 V
Based on the cell potential, what is the concentration of Cu^{2+}
in this solution?
[Cu2+]____ with units
PLEASE HELP ME!!
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