For the reaction taking place in the cell: Pt ( s )| H 2( g )| H +( aq ) | Ag+( aq ) mid Ag ( s ) E text Cell o =+0.5332 V. The value of Δ f G 0 is kJ mol -1. (in nearest integer)

Question

For the reaction taking place in the cell: Pt ( s )| H 2( g )| H +( aq ) | Ag+( aq ) mid Ag ( s ) E text Cell o =+0.5332 V. The value of Δ f G 0 is kJ mol -1. (in nearest integer) (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

(1/2) H 2+ Ag + arrow H ++ Ag Δ G °=- nE ° F =-1 × 0.5332 × 96500 J =-51.35 kJ ( n =2. for .H 2+2 Ag + arrow 2 H ++2 Ag )

Q. For the reaction taking place in the cell: $Pt (s) ∣ H_{2} (g) ∣ H^{+} (a q) ∥ A g^{+} (a q) ∣ A g (s)$ $E_{Cell}^{o} = + 0.5332 V$ .
The value of $Δ_{f} G^{0}$ is ___ $k J m o l^{- 1}$ . (in nearest integer)

$\frac{1}{2} H_{2} + A g^{+} \to H^{+} + A g$
$Δ G^{\circ} = - n E^{\circ} F$
$= - 1 \times 0.5332 \times 96500 J$
$= - 51.35 k J$
$(n = 2$ for $H_{2} + 2 A g^{+} \to 2 H^{+} + 2 A g)$

Q. For the reaction taking place in the cell: Pt(s)∣H2​(g)∣H+(aq)∥Ag+(aq)∣Ag(s) ECell o​=+0.5332V. The value of Δf​G0 is ___kJmol−1. (in nearest integer)

21​H2​+Ag+→H++Ag ΔG∘=−nE∘F =−1×0.5332×96500J =−51.35kJ (n=2 for H2​+2Ag+→2H++2Ag)

Q. For the reaction taking place in the cell: $Pt (s) ∣ H_{2} (g) ∣ H^{+} (a q) ∥ A g^{+} (a q) ∣ A g (s)$ $E_{Cell}^{o} = + 0.5332 V$ .
The value of $Δ_{f} G^{0}$ is ___ $k J m o l^{- 1}$ . (in nearest integer)

$\frac{1}{2} H_{2} + A g^{+} \to H^{+} + A g$
$Δ G^{\circ} = - n E^{\circ} F$
$= - 1 \times 0.5332 \times 96500 J$
$= - 51.35 k J$
$(n = 2$ for $H_{2} + 2 A g^{+} \to 2 H^{+} + 2 A g)$