Consider an electrochemical cell: A(s)|An+(aq,2M)||B2n+(aq,1M)|B(s). The value of ΔH0for the cell reaction is thrice that of ΔG0 at 300 K. If the emf of the cell is zero, the ΔS0 in J K–1mol–1 of the cell reaction per mole of B formed at 300 K is: Given:ln(2)=0.7,R=8.3 JK–1mol–1. H, S and G are enthalpy, entropy and Gibbs energy, respectively.

Consider an electrochemical cell: A(s)|An+(aq,2M)||B2n+(aq,1M)|B(s)

1.	Consider an electrochemical cell: A(s)\|An+(aq,2M)\|\|B2n+(aq,1M)\|B(s). The value of ΔH0for the cell reaction is thrice that of ΔG0 at 300 K. If the emf of the cell is zero, the ΔS0 in J K–1mol–1 of the cell reaction per mole of B formed at 300 K is: Given:ln(2)=0.7,R=8.3 JK–1mol–1. H, S and G are enthalpy, entropy and Gibbs energy, respectively.
Answer» Consider an electrochemical cell: $A (s) \| A^{n +} (a q, 2 M) \| \| B^{2 n +} (a q, 1 M) \| B (s) .$ The value of $Δ H^{0}$ for the cell reaction is thrice that of $Δ G^{0}$ at 300 K. If the emf of the cell is zero, the $Δ S^{0}$ in $J K^{- 1} m o l^{- 1}$ of the cell reaction per mole of B formed at 300 K is: Given: $l n (2) = 0.7$ , $R = 8.3 J K^{- 1} m o l^{- 1}$ . H, S and G are enthalpy, entropy and Gibbs energy, respectively.