Determine the standard reduction potential for the half cell reaction, Cl 2+2 e- arrow 2 Cl - given, Pt 2++2 Cl - arrow Pt + Cl 2, E text cell °=-0.15 V Pt 2++2 e- arrow Pt , E°=1.20 V

Question

Determine the standard reduction potential for the half cell reaction, Cl 2+2 e- arrow 2 Cl - given, Pt 2++2 Cl - arrow Pt + Cl 2, E text cell °=-0.15 V Pt 2++2 e- arrow Pt , E°=1.20 V  (A) 1.05 V (B) -1.05 V (C) -1.35 V (D) 1.35 V

Tardigrade Admin · Accepted Answer

Pt + Cl 2 arrow Pt 2++2 Cl - ; E Cell °=0.15 V (i) Pt 2++2 e- arrow Pt ; E° Cell =1.20 V (ii) Addition, Cl 2+2 e- arrow 2 Cl - ; E°=0.15+1.20=1.35 V

Q. Determine the standard reduction potential for the half cell reaction, $C l_{2} + 2 e^{-} \to 2 C l^{-}$
given, $P t^{2 +} + 2 C l^{-} \to Pt + C l_{2}, E_{cell}^{\circ} = - 0.15 V$
$P t^{2 +} + 2 e^{-} \to Pt, E^{\circ} = 1.20 V$

1.05 V

-1.05 V

-1.35 V

1.35 V

$Pt + C l_{2} \to P t^{2 +} + 2 C l^{-}; E_{C e ll}^{\circ} = 0.15 V (i)$

$P t^{2 +} + 2 e^{-} \to Pt; E^{\circ} C e ll = 1.20 V (ii)$

Addition, $C l_{2} + 2 e^{-} \to 2 C l^{-}; E^{\circ} = 0.15 + 1.20 = 1.35 V$

Q. Determine the standard reduction potential for the half cell reaction, Cl2​+2e−→2Cl− given, Pt2++2Cl−→Pt+Cl2​,Ecell ∘​=−0.15V Pt2++2e−→Pt,E∘=1.20V