ElectrochemistryEasy
Question
Standard reduction potentials of the half reactions are given below:
F2(g) + 2e- → 2F-(aq) ; Eo = + 2.85 V
Cl2(g) 2e- → 2Cl-(aq) ; Eo = + 1.36 V
Br2(g) + 2e- → 2Br-(aq) ; Eo = + 1.06 V
I2(g) + 2e- → 2I-(aq) ; Eo = + 0.53 V
The strongest oxidising and reducing agents respectively are:
F2(g) + 2e- → 2F-(aq) ; Eo = + 2.85 V
Cl2(g) 2e- → 2Cl-(aq) ; Eo = + 1.36 V
Br2(g) + 2e- → 2Br-(aq) ; Eo = + 1.06 V
I2(g) + 2e- → 2I-(aq) ; Eo = + 0.53 V
The strongest oxidising and reducing agents respectively are:
Options
A.Cl2 and I2
B.F2 and I-
C.Br2 and Cl-
D.Cl2 and Br-
Solution
F2 + 2e- → 2F-(aq); Eo = + 2.85 V
I2 + 2e- → 2I-(aq); Eo = + 0.53 V
F2 with highest reduction potential is the strongest oxidising agent.
I2 + 2e- → 2I-(aq); Eo = + 0.53 V
F2 with highest reduction potential is the strongest oxidising agent.
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