1. Tardigrade
  2. Question
  3. Chemistry
  4. Consider the following standard electrode potentials and calculate the equilibrium constant at 25° C for the indicated disproportionation reaction: 3 Mn 2+( aq ) longrightarrow Mn ( s )+2 Mn 3+( aq ) Mn 3+( aq )+ e - longrightarrow Mn 2+( aq ) ; E°=1.51 V Mn 2+( aq )+2 e - longrightarrow Mn ( s ) ; E°=-1.185 V

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Q. Consider the following standard electrode potentials and calculate the equilibrium constant at $25^{\circ} C$ for the indicated disproportionation reaction :
$3 Mn ^{2+}( aq ) \longrightarrow Mn ( s )+2 Mn ^{3+}( aq ) $
$Mn ^{3+}( aq )+ e ^{-} \longrightarrow Mn ^{2+}( aq ) ; E^{\circ}=1.51 \,V$
$Mn ^{2+}( aq )+2 e ^{-} \longrightarrow Mn ( s ) ; \quad E^{\circ}=-1.185\, V$

Electrochemistry

Solution:

Correct answer is (c) $6.3 \times 10^{-92}$

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