1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
Shkiper50 [21]
3 years ago
12

An electrochemical cell at 25°C is composed of pure copper and pure lead solutions immersed in their respective ionis. For a 0.6

M concentration of Cu2+, the lead electrode is oxidized yielding potential of 0.507 V. a cell a) Calculate the concentration of Pb2+ b) Suppose the lead electrode is reduced, in that case what would be the concentration of Pb2 What does this answer tell you?
Chemistry
1 answer:
ExtremeBDS [4]3 years ago
6 0

Answer :

(a) The concentration of Pb^{2+} is, 0.0337 M

(b) The concentration of Pb^{2+} is, 6.093\times 10^{32}M

Solution :

<u>(a) As per question, lead is oxidized and copper is reduced.</u>

The oxidation-reduction half cell reaction will be,

Oxidation half reaction:  Pb\rightarrow Pb^{2+}+2e^-

Reduction half reaction:  Cu^{2+}+2e^-\rightarrow Cu

The balanced cell reaction will be,  

Pb(s)+Cu^{2+}(aq)\rightarrow Pb^{2+}(aq)+Cu(s)

Here lead (Pb) undergoes oxidation by loss of electrons, thus act as anode. Copper (Cu) undergoes reduction by gain of electrons and thus act as cathode.

First we have to calculate the standard electrode potential of the cell.

E^o_{[Pb^{2+}/Pb]}=-0.13V

E^o_{[Cu^{2+}/Cu]}=+0.34V

E^o=E^o_{[Cu^{2+}/Cu]}-E^o_{[Pb^{2+}/Pb]}

E^o=0.34V-(-0.13V)=0.47V

Now we have to calculate the concentration of Pb^{2+}.

Using Nernest equation :

E_{cell}=E^o_{cell}-\frac{0.0592}{n}\log \frac{[Pb^{2+}]}{[Cu^{2+}]}

where,

n = number of electrons in oxidation-reduction reaction = 2

E_{cell} = 0.507 V

Now put all the given values in the above equation, we get:

0.507=0.47-\frac{0.0592}{2}\log \frac{[Pb^{2+}]}{(0.6)}

[Pb^{2+}]=0.0337M

Therefore, the concentration of Pb^{2+} is, 0.0337 M

<u>(b) As per question, lead is reduced and copper is oxidized.</u>

The oxidation-reduction half cell reaction will be,

Oxidation half reaction:  Cu\rightarrow Cu^{2+}+2e^-

Reduction half reaction:  Pb^{2+}+2e^-\rightarrow Pb

The balanced cell reaction will be,  

Cu(s)+Pb^{2+}(aq)\rightarrow Cu^{2+}(aq)+Pb(s)

Here Copper (Cu) undergoes oxidation by loss of electrons, thus act as anode. Lead (Pb) undergoes reduction by gain of electrons and thus act as cathode.

First we have to calculate the standard electrode potential of the cell.

E^o_{[Pb^{2+}/Pb]}=-0.13V

E^o_{[Cu^{2+}/Cu]}=+0.34V

E^o=E^o_{[Pb^{2+}/Pb]}-E^o_{[Cu^{2+}/Cu]}

E^o=-0.13V-(0.34V)=-0.47V

Now we have to calculate the concentration of Pb^{2+}.

Using Nernest equation :

E_{cell}=E^o_{cell}-\frac{0.0592}{n}\log \frac{[Cu^{2+}]}{[Pb^{2+}]}

where,

n = number of electrons in oxidation-reduction reaction = 2

E_{cell} = 0.507 V

Now put all the given values in the above equation, we get:

0.507=-0.47-\frac{0.0592}{2}\log \frac{(0.6)}{[Pb^{2+}]}

[Pb^{2+}]=6.093\times 10^{32}M

Therefore, the concentration of Pb^{2+} is, 6.093\times 10^{32}M

You might be interested in
HELP
Vesnalui [34]

Answer:

145.8g

Explanation:

Given parameters:

Number of moles of magnesium hydroxide  = 2.5mol

Unknown:

Mass of Mg(OH)₂  = ?

Solution:

To solve this problem we use the expression below;

  Mass of Mg(OH)₂ = number of moles x molar mass

 Molar mass of Mg(OH)₂ = 24.3 + 2(16 + 1)  = 58.3g/mol

 Mass of Mg(OH)₂ = 2.5 x 58.3  = 145.8g

3 0
2 years ago
Organisms breakdown _____ in order to produce____?
Novay_Z [31]

Answer: Organisms breakdown __into smaller particles___ in order to produce__new compounds__?

Explanation:

branliest pls :)

3 0
2 years ago
Read 2 more answers
Granite is a ________ that contains the mineral quartz. a. mineral c. rock b. glass d. mica
kow [346]
I think it would be C

7 0
3 years ago
Read 2 more answers
A mixture of 10.0 g of Ne and 10.0 g Ar have a total pressure of 1.6 atm. What is the partial pressure of Ne?
Natasha2012 [34]
If u add u will get ur answer
7 0
3 years ago
Read 2 more answers
What is the percent error if the measured value is 30.0 g and<br> the accepted value is 32.0 g?
JulsSmile [24]

Answer:6.25

Explanation:

3 0
3 years ago
Other questions:
  • Calculate the number of kilojoules to warm 125 g of iron from 23.5 °C to 78.0 °C.
    7·1 answer
  • What bonds break? select that apply
    7·1 answer
  • Why was it possible to neutralize HCI using NaOH?
    6·1 answer
  • Organisms with traits that are well-suited to an environment tend to survive and reproduce at a greater rate than organisms that
    8·1 answer
  • Most people now know that hot air____ as a result of its lower density.
    15·1 answer
  • Camphor (C10H16O) melts at 179.8°C, and it has a particularly large freezing-point-depression constant, Kf= 40.0ºC/m. When 0.186
    11·2 answers
  • ___ is anything that has mass and volume<br>Pls help
    12·2 answers
  • The diagram shows an electric motor.
    13·2 answers
  • Where do plants get their energy?
    6·1 answer
  • A. Identify which sets of quantum numbers are valid for an electron. Each set is ordered (n,ℓ,mℓ,ms).
    12·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!