ElectrochemistryHard
Question
At what pH does the potential (EMF) for the disproportionation of chlorine change from a negative value to a positive value, assuming 1.0 bar pressure and 1.0 M concentration for all species except hydrogen ion?
Given: Cl2 + 2e− → 2Cl−; E° = 1.36 V
2OCl− + 4H+ + 2e− → Cl2 + 2H2O; E° = 1.63 V.
[2.303 RT/F = 0.06]
Options
A.4.5
B.1.5
C.2.25
D.9.0
Solution
$Cl_{2} + H_{2}O \rightleftharpoons Cl^{-} + ClO^{-} + 2H^{+}$
$E_{cell}^{o} = 1.36 - 1.63 = - 0.27\text{ V} $$${\text{Now, }E_{cell} = E_{cell}^{o} - \frac{0.06}{1}{\log\left\lbrack H^{+} \right\rbrack}^{2} }{\text{Or, 0 = } - 0.27 + \frac{0.06}{1} \times 2P^{H} = 2.25}$$
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