The standard redox potential for reactions Mn 2-2 e - Mn and Mn 3-1 e - Mn 2- are 2-36 and 1-51 V respectively - What is the redox potential for the reaction Mn 3-3 e - Mn -

Mn2++2e —– gt; Mn ——(1) standard redox potential.E01=2.36V Mn3+ +1e —– gt; Mn2+——(2) standard redox potential.E1=1.51V (1)+(2) = g ...

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Oxidising and Reducing Nature

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The standard redox potential for reactions Mn²⁺+2e -----> Mn and Mn³⁺+1e -----> Mn²⁺ are 2.36 and 1.51V respectively . What is the redox potential for the reaction Mn³⁺+3e------> Mn ?

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M n^{2 +} + 2 e^{-} \to M n; E^{0} = - 1.18 V

2 (M n^{3 +} + e^{-} \to M n^{2 +}); E^{0} = + 1.51 V

E^{0}

3 M n^{2 +} \to M n + 2 M n^{3 +}

25^{\circ} C

M n O_{2} \to M n^{3 +}

E^{⊖} = 0.95 V

M n^{3 +} \to M n^{2 +}

E^{⊖} = 1.51 V

M n O_{2} \to M n^{2 +}

{M n}^{3 +}

M n = 55

{M n}^{3 +} ⟶ {M n}^{2 +} + M n O_{2}

E_{R P}^{o}

M n O_{4}^{-} (a q) + 8 H^{+} + 5 e \to M n^{2 +} (a q) + 4 H_{2} O (l); E^{o} = + 1.52 V

M n O_{4}^{2 -} (a q) + 4 H^{+} + 2 e \to M n O_{2} (s) + 2 H_{2} O (l); E^{o} = + 2.26 V

2 M n O_{4}^{-} (a q) + 2 e \to 2 M n O_{4}^{2 -} (a q); E^{o} = + 0.56 V

M n^{3 +} + e \to M n^{2 +}; E^{o} = + 1.51 V

M n^{4 +} + e \to M n^{3 +}; E^{o} = 0.95 V

M n^{2 +} + 2 e^{-} \to M n; E^{\circ} = - 1.18 V

2 (M n^{3 +} + e^{-} \to M n^{2 +}); E^{\circ} = + 1.51 V

E^{\circ}

3 M n^{2 +} \to M n + 2 M n^{3 +}

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