The Gibbs energy change (in J) for the given reaction at [ Cu 2+]=[ Sn 2+]=1 M and 298 K is: Cu ( s )+ Sn 2+( aq .) arrow Cu 2+( aq .)+ Sn ( s ) ( E Sn 2+ Sn 0=-0.16 V , E Cu 2+| Cu 0=0.34 V . Take .F=96500 C mol -1)

Question

The Gibbs energy change (in J) for the given reaction at [ Cu 2+]=[ Sn 2+]=1 M and 298 K is: Cu ( s )+ Sn 2+( aq .) arrow Cu 2+( aq .)+ Sn ( s ) ( E Sn 2+ Sn 0=-0.16 V , E Cu 2+| Cu 0=0.34 V . Take .F=96500 C mol -1) (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

Δ G=Δ Go+R T ln [(S n+2/C u+2)] =-2 × 96500[(-0.16)-0.34]+R T ln ((1/1)) =96500 J

Q. The Gibbs energy change (in J) for the given reaction at $[C u^{2 +}] = [S n^{2 +}] = 1 M$ and $298 K$ is:

$C u (s) + S n^{2 +} (a q .) \to C u^{2 +} (a q .) + S n (s)$

$(E_{S n^{2 +} S n}^{0} = - 0.16 V, E_{C u^{2 +} ∣ C u}^{0} = 0.34 V$

Take $F = 96500 C m o l^{- 1})$

$Δ G = Δ G^{o} + RT ln [\frac{S n ^{+ 2}}{C u ^{+ 2}}]$

$= - 2 \times 96500 [(- 0.16) - 0.34] + RT ln (\frac{1}{1})$

$= 96500 J$

Q. The Gibbs energy change (in J) for the given reaction at [Cu2+]=[Sn2+]=1M and 298K is: Cu(s)+Sn2+(aq.)→Cu2+(aq.)+Sn(s) (ESn2+Sn0​=−0.16V,ECu2+∣Cu0​=0.34V Take F=96500Cmol−1)

ΔG=ΔGo+RTln[Cu+2Sn+2​] =−2×96500[(−0.16)−0.34]+RTln(11​) =96500J

Q. The Gibbs energy change (in J) for the given reaction at $[C u^{2 +}] = [S n^{2 +}] = 1 M$ and $298 K$ is:

$C u (s) + S n^{2 +} (a q .) \to C u^{2 +} (a q .) + S n (s)$

$(E_{S n^{2 +} S n}^{0} = - 0.16 V, E_{C u^{2 +} ∣ C u}^{0} = 0.34 V$

Take $F = 96500 C m o l^{- 1})$

$Δ G = Δ G^{o} + RT ln [\frac{S n ^{+ 2}}{C u ^{+ 2}}]$

$= - 2 \times 96500 [(- 0.16) - 0.34] + RT ln (\frac{1}{1})$

$= 96500 J$