Δ Go of the cell reaction AgCl (s) + (1/2) H2 (g) = Ag (s) + H+ + Cl- is -21.52 kJ. Δ Go of 2AgCl (s) + H2 (g) = 2Ag (s) + 2H+ + 2Cl- is

Question

Δ Go of the cell reaction AgCl (s) + (1/2) H2 (g) = Ag (s) + H+ + Cl- is -21.52 kJ. Δ Go of 2AgCl (s) + H2 (g) = 2Ag (s) + 2H+ + 2Cl- is (A) -21.52 kJ (B) -10.76 kJ (C) -43.04 kJ (D) 43.04 kJ

Tardigrade Admin · Accepted Answer

KC2=KC12 ∴ Δ G=-nfEo=-RT ln Kc ∴ G2 =2×(-21.52)=-43.04 KJ

Q. $Δ G^{o}$ of the cell reaction
$A g Cl (s) + \frac{1}{2} H_{2} (g) = A g (s) + H^{+} + C l^{-} i s - 21.52 k J .$
$Δ G^{o}$ of $2 A g Cl (s) + H_{2} (g)$ = $2 A g (s) + 2 H^{+} + 2 C l^{-}$ is

$- 21.52 k J$

$- 10.76 k J$

$- 43.04 k J$

$43.04 k J$

$K_{C_{2}} = K_{C_{1}}^{2}$
$∴ Δ G = - n f E_{o} = - RTl n K_{c}$
$∴ G_{2} = 2 \times (- 21.52) = - 43.04 K J$

Q. ΔGo of the cell reaction AgCl(s)+21​H2​(g)=Ag(s)+H++Cl−is−21.52kJ. ΔGo of 2AgCl(s)+H2​(g) = 2Ag(s)+2H++2Cl− is

−21.52kJ

−10.76kJ

−43.04kJ

43.04kJ