Question

The standard reduction potential for the half cell reaction $Cl_{} + 2e^{-} \rightarrow 2Cl^{-}$will be

($Pt^{2 +} + 2Cl^{-} \rightarrow Pt + Cl_{2},Eº_{Cell} = - 0.15V;$

$Pt^{2 +} + 2e^{-} \rightarrow Pt,Eº = 1.20V$)

• A. $- 1.35V$
• B. $+ 1.35V$
• C. $- 1.05V$
• D. $+ 1.05V$

Answer 1

Answer: (B)

$+ 1.35V$

Answer 2

$Pt + Cl_{2} \rightarrow Pt^{2} + 2Cl^{-};Eº_{cell} = 0.15V$

$Pt^{2} + 2e^{-} \rightarrow Pt;Eº = 1.20V$

$Cl_{2} + 2e^{-} \rightarrow 2Cl^{-};Eº = 1.35$