reduction table

Electrochemistry : Standard Reduction Potentials

Standard Reduction Potentials
in Aqueous Solution at 25C

	Half-reaction				E (V)
	Li⁺ + e^-		Li_(s)		-3.05	Best Reducing Agents
	Cs⁺ + e^-		Cs_(s)		-2.92
	K⁺ + e^-		K_(s)		-2.92
	Rb⁺ + e^-		Rb_(s)		-2.92
	Ba²⁺ + 2 e^-		Ba_(s)		-2.90
	Sr²⁺ 2 e^-		Sr_(s)		-2.89
	Ca²⁺ + 2 e^-		Ca_(s)		-2.87
	Na⁺ + e^-		Na_(s)		-2.71
	Mg²⁺ + 2 e^-		Mg_(s)		-2.37
	Be²⁺ + 2 e^-		Be_(s)		-1.70
	Al³⁺ + 3 e^-		Al_(s)		-1.66
	Mn²⁺ + 2 e^-		Mn_(s)		-1.18
	Zn²⁺ + 2 e^-		Zn_(s)		-0.76
	Cr³⁺ + 3 e^-		Cr_(s)		-0.74
	Fe²⁺ + 2 e^-		Fe_(s)		-0.44
	Cr³⁺ + e^-		Cr²⁺		-0.41
	Cd²⁺ + 2 e^-		Cd_(s)		-0.40
	Tl⁺ + e^-		Tl_(s)		-0.34
	Co²⁺ + 2 e^-		Co_(s)		-0.28
	Ni²⁺ + 2 e^-		Ni_(s)		-0.25
Oxidizing power increases	Sn²⁺ + 2e^-		Sn_(s)		-0.14	Reducing power increases
	Pb²⁺+ 2 e^-		Pb_(s)		-0.13
	2 H⁺ + 2 e^-		H_2(g)		0.00
	S_(s) + 2 H⁺ + 2 e^-		H₂S _(g)		0.14
	Sn⁴⁺ + 2 e^-		Sn²⁺		0.15
	Cu²⁺ + e^-		Cu⁺		0.15
	Cu²⁺ + 2 e^-		Cu_(s)		0.34
	Cu⁺ + e^-		Cu_(s)		0.52
	I_2(s) + 2 e^-		2 I^-		0.53
	Fe³⁺ + e^-		Fe²⁺		0.77
	Hg₂²⁺ + 2 e^-		2 Hg_(l)		0.79
	Ag⁺ + e^-		Ag_(s)		0.80
	Hg²⁺ + 2 e^-		Hg_(l)		0.85
	2 Hg²⁺ + 2 e^-		Hg₂²⁺		0.92
	Br_2(l) + 2 e		2 Br^-		1.07
	O_2(g) + 4 H⁺ + 4 e^-		2 H₂O_(l)		1.23
Best Oxidizing Agents	Cl_2(g) + 2 e^-		2 Cl^-		1.36
	Au³⁺ + 3 e^-		Au_(s)		1.50
	Co³⁺ + e^-		Co²⁺		1.82
	F_2(g) + 2 e^-		2 F^-		2.87