Question
In: Chemistry
A voltaic cell is constructed using solutions of NaHSO4, H2SO3, and MnSO4 with suitable electrodes. The...
A voltaic cell is constructed using solutions of NaHSO4, H2SO3, and MnSO4 with suitable electrodes. The relevant half reactions are:
HSO4- (aq) + 3H+ (aq) +2e- --> H2SO3(aq) + H2O (E0= 0.17v)
Mn+2(aq) + 2e- --> Mn(s) (E0= -1.18v)
A. Write the equation for the overall cell reaction and calculate the cell potential at standard conditions.
B. Calculate the cell potential if the [H+] is changed to pH=1.
C. Predict the qualitative effect (increase, decrease,no change) and order of magnitude (significant,minimal) on the cell potential if a solution of Ba(NO3)2 is added to both cell compartments. Explain your prediction.
BaSO3 Ksp= 8.3 x 10-7
BaSO4 Ksp= 1.2 x 10-10
Solutions
Expert Solution
HSO4- (aq) + 3H+ (aq) +2e- --> H2SO3(aq) + H2O (E0= 0.17v)
Mn+2(aq) + 2e- --> Mn(s) (E0= -1.18v)
Mn(s) ------------------------> Mn^2+ (aq) + 2e^- E0 = 1.18v
HSO4- (aq) + 3H+ (aq) +2e- --> H2SO3(aq) + H2O (E0= 0.17v)
--------------------------------------------------------------------------------------------------
Mn(s) +HSO4- (aq) + 3H+ (aq) --> Mn^2+(aq) +H2SO3(aq) + H2O E0cell = 1.35v
B. PH = 1
-log[H+] = 1
[H+] = 10^-1M
queen_honey_blossom answered 2 years agoRelated Solutions
A voltaic cell is constructed with two silver-silver chloride electrodes, each of which is based on...
A voltaic cell is constructed with two silver-silver chloride
electrodes, each of which is based on the following half-reaction:
AgCl(s)+e−→Ag(s)+Cl−(aq). The two cell compartments have [Cl−]=
1.60×10−2 M and [Cl−]= 3.00 M , respectively.
Which electrode is the cathode of the cell?
the compartment with 1.60×10−2 M
Cl(aq) is the
cathode
Correct
2. What is the standard emf of the cell?
3.What is the cell emf for the concentrations given?
4. For the anode compartment, predict whether [Cl−] will
increase,...
A voltaic cell is constructed with two silver-silver chloride electrodes, each of which is based on...
A voltaic cell is constructed with two silver-silver chloride
electrodes, each of which is based on the following
half-reaction:
AgCl(s)+e−→Ag(s)+Cl−(aq).
The two cell compartments have [Cl−]=1.49×10−2 M and
[Cl−]= 3.00 M , respectively.
a. Which electrode is the cathode of the cell?
b. What is the standard emf of the cell?
c. What is the cell emf for the concentrations given?
d. For the anode compartment, predict whether [Cl−] will
increase, decrease, or stay the same as the cell operates....
A voltaic cell is constructed using a Sn electrode in .50 M SnSO4 and a Cd...
A voltaic cell is constructed using a Sn electrode in .50 M
SnSO4 and a Cd electrode in .01M CdSO4 solution. Determine the
following:
a) Overall reaction
b) Metal oxidized
c) Metal Reduced
d) E0 cell
e) E cell
A voltaic cell is constructed using the reaction of chromium metal and iron(II) ion: &nb
A voltaic cell is constructed using the reaction of chromium
metal and iron(II)
ion:
2Cr(s) +3Fe2+(aq) ®
2Cr3+(aq) +3Fe(s)
What is the correct cell notation for this voltaic cell?
Which insoluble compound in each pair should be more soluble in
nitric acid than in pure water?
a) PbCl2 or PbS
b) Ag2CO3 or AgI
c) Al(OH)3 or AgCl
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...
A voltaic cell similar to that shown in Figure 20.5 in the textbook is constructed. One...
A voltaic cell similar to that shown in Figure 20.5 in the
textbook is constructed. One electrode compartment consists of a
silver strip placed in a solution of AgNO3, and the other has an
iron strip placed in a solution of FeCl2. The overall cell reaction
is Fe(s)+2Ag+(aq)?Fe2+(aq)+2Ag(s) You may want to reference (Pages
858 - 859) Section 20.3 while completing this problem.
Part A
What species is oxidized?
Express your answer as a species from the balanced chemical
equation....
Identify the anode in a galvanic cell of copper and brass electrodes in standard solutions of...
Identify the anode in a galvanic cell of copper and brass
electrodes in standard solutions of their own ions. Identify the
anode in a galvanic cell of a two-phase microstructure of a 50:50
Pb-Sn alloy. Identify the anode in a galvanic cell of a lead-tin
solder on a Cast iron in seawater. Identify the anode in a galvanic
cell of a brass bolt in a passive 430 stainless steel plate in
seawater.
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 voltaic cell is constructed that uses the following reaction and operates at 298 K. Zn(s)...
A voltaic cell is constructed that uses the following reaction
and operates at 298 K. Zn(s) + Ni2+(aq) Zn2+(aq) + Ni(s) (a)
What is the emf of this cell under standard conditions?______
V
(b) What is the emf of this cell when [Ni2+] = 2.24 M and [Zn2+]
= 0.112 M?_____ V
(c) What is the emf of the cell when [Ni2+] = 0.298 M and [Zn2+]
= 0.925 M?____ V
ADVERTISEMENT
ADVERTISEMENT
Latest Questions
- an investment pays 2600 per year for the first 7 years, 5200 per year for the...
- Portsmouth Company makes upholstered furniture. Its only variable cost is direct materials. The demand for the...
- C++ How would I sort my output to evaluate it by sorting the column by it's...
- A cake is shaped like a hemisphere of radius 2 with its base on the xy-plane....
- Explain the similarities and differences between spiders, crawlers and bots in relation to search engines. Additionally...
- ] How much weight do you have to invest in KLM in order to earn the...
- Cpp challenge Description The purpose of this challenge is to use the WHILE loop to control...
ADVERTISEMENT