This document discusses how to write cell reactions and calculate standard reduction potentials using the Nernst equation. It begins by explaining how to write the cell reaction for a Daniell cell, including identifying the anode and cathode half-reactions. It then shows how to write the overall cell reaction and standard cell notation. Finally, it demonstrates calculating the standard reduction potential using the Nernst equation with an example.
3. How do we write a cell reaction?
Lets start with the Construction of Daniell cell:
4. How do we write a cell reaction?
Lets start with the Construction of Daniell cell:
Can you mention
the anode and
cathode?
5. How do we write a cell reaction?
The cell reaction is as follows:
• This cell converts the chemical
energy liberated during the redox
reaction into electrical energy.
• If an external opposite potential
is applied and increased slowly, we
find that the reaction continues to
take place till the opposing voltage
reaches the value 1.1 V.
• The reaction stops altogether and no
current flows through the cell.
6. How do we write a cell reaction?
The cell reaction is as follows:
• Zn(s) + Cu2+(aq) → Zn2+ (aq) + Cu(s)
What do we write
standard form of
cell reaction?
7. How do we write a cell reaction?
The cell reaction is as follows:
• Zn(s) + Cu2+(aq) → Zn2+ (aq) + Cu(s)
Zn | Zn2+ || Cu2+ | Cu
Let us consider the left-hand side of the standard cell.
Zn | Zn2+
• The Left-hand side is always the anode.
• Oxidation takes place at the anode.
• The half-cell with the more negative potential is always
taken as the anode.
• In oxidation there is always loss of electrons.
Therefore the oxidation half-cell reaction is:
Zn → Zn2+ + 2e-
8. How do we write a cell reaction?
The cell reaction is as follows:
• Zn(s) + Cu2+(aq) → Zn2+ (aq) + Cu(s)
Zn | Zn2+ || Cu2+ | Cu
Let us consider the left-hand side of the standard cell.
Cu2+| Cu
• The Right-hand side is always the cathode.
• Reduction takes place at the cathode.
• The half-cell with the more positive potential is always
taken as the cathode.
• In reduction there is always gain of electrons.
Therefore the reduction half-cell reaction is:
Cu2+ + 2e- → Cu
9. How do we write a cell reaction?
So how do we
write the overall
cell reaction?
10. How do we write a cell reaction?
We know that:
Oxidation Reaction: Zn → Zn2+ + 2e-
Reduction Reaction: Cu2+ + 2e- → Cu
So, for overall reaction we add both the reactions
together.
The 2 electrons on both the sides of the half-cell get
cancelled.
Overall Reaction: Zn(s) + Cu2+(aq) → Zn2+ (aq) + Cu(s)
11. How do we write a cell reaction?
Let us solve some examples:
12. How do we write a cell reaction?
Let us solve some examples:
13. How do we write a cell reaction?
Let us solve some examples:
14. How do we calculate the standard
reduction potential?
The standard reduction potential is given by:
E0
cell= Ecathode - E
The reduction potential of the cell is given by the nernst
equation:
15. What do we calculate the standard
reduction potential?
Let us go through an example:
16. What do we calculate the standard
reduction potential?
Let us go through an example:
Can you write
the standard
cell reaction?
17. What do we calculate the standard
reduction potential?
Let us go through an example:
Can you write the
overall reaction
along with
the half-cell
reaction?
18. What do we calculate the standard
reduction potential?
Let us go through an example:
Can you solve
using the nernst
equation and find
the standard
reduction
potential?
19. What do we calculate the standard
reduction potential?
Let us go through an example:
20. What do we calculate the standard
reduction potential?
Let us go through an example:
=
21. What do we calculate the standard
reduction potential?
Let us go through an example:
=
=
22. What do we calculate the standard
reduction potential?
Let us solve some examples:
1.
2.
3.
23. Learning Outcomes
• To solve numericals on cell reaction and Nernst equation.
How confident do you feel?
24. Learning Outcomes
• To solve numericals on cell reaction and Nernst equation.
How confident do you feel?
Editor's Notes
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