• Based on the following electrochemical cell notation: Fe (s/ Fe2* (ag) I| MnO4 (aq), II MnOA (aq) ' H* (aq) , Mn2" (aq) / Pts) * Write the balanced overall reaction for the above cell. i Sketch a labelled diagram for the cell. iii) Determine the equilibrium constant for the cell.

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Chapter1: Chemical Foundations
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Based on the following electrochemical cell
notation:
Fe (s)/ Fe2+
II MnOA (aq) :
(aq)
Mn2+,
H (aq) '
(aq)/ Pt(s)
* Write the balanced overall reaction for the above
cell.
i Sketch a labelled diagram for the cell.
iii)
Determine the equilibrium constant for the cell.
iv)
Identify the oxidizing agent and reducing agent.
Calculate the cell potential when [Fe2*]=0.1M,
[MnO,1=0.2M, [Mn2+]=0.5M in pH 4 solution at
30°C.
v)
vi) Determine the Free Gibb's energy to indicate its
spontaneity.
(Faraday's constant = 96500 C/mol, Gas ideal constant,
R= 8.314 J/K.mol)
Transcribed Image Text:Based on the following electrochemical cell notation: Fe (s)/ Fe2+ II MnOA (aq) : (aq) Mn2+, H (aq) ' (aq)/ Pt(s) * Write the balanced overall reaction for the above cell. i Sketch a labelled diagram for the cell. iii) Determine the equilibrium constant for the cell. iv) Identify the oxidizing agent and reducing agent. Calculate the cell potential when [Fe2*]=0.1M, [MnO,1=0.2M, [Mn2+]=0.5M in pH 4 solution at 30°C. v) vi) Determine the Free Gibb's energy to indicate its spontaneity. (Faraday's constant = 96500 C/mol, Gas ideal constant, R= 8.314 J/K.mol)
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