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Consider an electrochemical cell : A((s)...

Consider an electrochemical cell : `A_((s))|A^(n+)((aq,2M)||B^(2n+) ((aq,1M)|B_(s)` The value of `DeltaH^(@)` for the cell reaction is twice that of `DeltaG^(@)` at 300K . If the emf of the cell is zero, the `DeltaS^(@)` (in JK^(-1mol^(-1))` of the cell reaction per mole of B formed at 300 K is _________.
(Given ln (2)= 0.7, R (universal gas constant ) = `8.3JK^(-1)mol^(-1)`. H, S and G are enthalpy , entropy and gibbs energy, respectively).

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To solve the problem, we need to analyze the information given about the electrochemical cell and apply the relevant thermodynamic equations. Here’s a step-by-step solution: ### Step 1: Understand the relationship between ΔH, ΔG, and ΔS We are given that ΔH = 2ΔG at 300 K. We also know from thermodynamics that: \[ \Delta G = \Delta H - T\Delta S \] Substituting ΔH = 2ΔG into the equation gives: ...
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