Give the standard electrode potentials-K-K - -2-93 V- Ag-Ag - -0-80 V- Cr-3-Cr - -0-74 VOut of these electrode which will be the strongest reducing agent- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp- nbsp-

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Gibb's Energy and Nernst Equation

Give the stan...

Question

Give the standard electrode potentials:
K⁺/K = -2.93 V, Ag⁺/Ag = +0.80 V, Cr⁺³/Cr = -0.74 V
Out of these electrode which will be the strongest reducing agent?

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K^{+} / K = - 2.93 V, A g^{+} / A g = 0.80 V,

H g^{2 +} / H g = 0.79 V, M g^{2 +} / M g = - 2.37 V, C r^{3 +} / C r = - 0.74 V

K^{+} / K = - 2.93 V A g^{+} / A g = 0.80 V H g^{2 +} / H g = 0.79 V M g^{2 +} / M g = - 2.73 V C r^{3 +} / C r = - 0.74 V

Given the standard electrode potentials,

$\frac{K^{+}}{K} = - 2.93 V,$

$\frac{A g^{+}}{A g} = 0.80 V$

$\frac{H g^{2 +}}{H g} = 0.79 V,$

$\frac{M g^{2 +}}{M g} = - 2.37 V$

$\frac{C r^{3 +}}{C r} = - 0.74 V$

Arrange these metals in their increasing order of reducing power.

K^{+} + e^{-} \to K; E^{0} = - 2.93 V A g^{+} + e^{-} \to A g; E^{0} = 0.80 V H g_{2}^{2 +} + e^{-} \to 2 H g; E^{0} = 0.79 V M g^{2 +} + e^{-} \to M g; E^{0} = - 2.37 V C r^{3 +} + e^{-} \to C r; E^{0} = - 0.74 V

The standard electrode potentials, K⁺/K= -2.93V, Ag⁺/Ag = 0.80V, the electrode which is negatively charged is

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