ΔrG° for the cell with the cell reaction: Zn(s)+Ag2O(s)+H2O(l) → Zn2+(aq)+2Ag(s)+2OH-(aq) [E°Ag2 O/Ag=0.344 V, E°Zn2+/Zn=-0.76 V]

Question

ΔrG° for the cell with the cell reaction: Zn(s)+Ag2O(s)+H2O(l) → Zn2+(aq)+2Ag(s)+2OH-(aq) [E°Ag2 O/Ag=0.344 V, E°Zn2+/Zn=-0.76 V] (A) 2.13×105 J mol-1 (B) -2.13×105 J mol-1 (C) 1.06×105 J mol-1 (D) -1.06×105 J mol-1

Tardigrade Admin · Accepted Answer

E°cell=E°Ag2 O/Ag-E°Zn2+/Zn =0.344-(-0.76)=1.104 V Δ G°=-nFE°cell=-2×96500×1.104 =-2.13×105 J mol-1

Q. $Δ_{r} G^{\circ}$ for the cell with the cell reaction :
$Z n_{(s)} + A g_{2} O_{(s)} + H_{2} O_{(l)} \to Z n_{(a q)}^{2 +} + 2 A g_{(s)} + 2 O H_{(a q)}^{-}$
$[E_{A g_{2} O / A g}^{\circ} = 0.344 V, E_{Z n^{2 +} / Z n}^{\circ} = - 0.76 V]$

$2.13 \times 1 0^{5} J m o l^{- 1}$

$- 2.13 \times 1 0^{5} J m o l^{- 1}$

$1.06 \times 1 0^{5} J m o l^{- 1}$

$- 1.06 \times 1 0^{5} J m o l^{- 1}$

$E_{ce ll}^{\circ} = E_{A g_{2} O / A g}^{\circ} - E_{Z n^{2 +} / Z n}^{\circ}$
$= 0.344 - (- 0.76) = 1.104 V$
$Δ G^{\circ} = - n F E_{ce ll}^{\circ} = - 2 \times 96500 \times 1.104$
$= - 2.13 \times 1 0^{5} J m o l^{- 1}$

Q. Δr​G∘ for the cell with the cell reaction : Zn(s)​+Ag2​O(s)​+H2​O(l)​→Zn(aq)2+​+2Ag(s)​+2OH(aq)−​ [EAg2​O/Ag∘​=0.344V,EZn2+/Zn∘​=−0.76V]

2.13×105Jmol−1

−2.13×105Jmol−1

1.06×105Jmol−1

−1.06×105Jmol−1