For the hypothetical reaction A + B^x → A^x + B,E° = 1.19 V = and ΔG° = -115 kJ.For this reaction the value of x = .

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The value of x can be determined using the Nernst equation: E° = E° - (RT/nF)lnQ, where E° is the standard cell potential, E° is the cell potential under non-standard conditions, R is the gas constant, T is the temperature in Kelvin, n is the number of moles of electrons transferred in the balanced chemical equation, F is the Faraday constant, and Q is the reaction quotient. In this case, E° = 1.19 V, E° = 0 V (since the reaction is at equilibrium), R = 8.314 J/mol·K, T = 298 K, n = x, and F = 96,485 C/mol. Substituting these values into the Nernst equation and solving for x gives x = 1.

For the Hypothetical Reaction a + Bx → Ax

For the Hypothetical Reaction a + B^x → A^x