For the electrochemical cell, Cd(s)| Cd²⁺(aq)|| Co²⁺(aq)| Co(s), determine the equilibrium constant (K_eq)at 25°C for the reaction that occurs.

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Quizplus · Accepted Answer

The equilibrium constant (K_eq) for the reaction can be calculated using the Nernst equation:E°cell = E°red - E°oxidwhere E°cell is the standard cell potential, E°red is the standard reduction potential of the reduction half-reaction, and E°oxid is the standard oxidation potential of the oxidation half-reaction.For the given electrochemical cell, the reduction half-reaction is:Co²⁺(aq) + 2 e^- → Co(s)and the oxidation half-reaction is:Cd(s) → Cd²⁺(aq) + 2 e^-The standard reduction potentials for these half-reactions are:E°red = -0.28 VE°oxid = -0.40 VTherefore, the standard cell potential is:E°cell = E°red - E°oxid = -0.28 V - (-0.40 V) = 0.12 VThe equilibrium constant (K_eq) is related to the standard cell potential by the equation:K_eq = e^nE°cell/RTwhere n is the number of electrons transferred in the reaction, R is the gas constant (8.314 J/mol·K), and T is the temperature in Kelvin (25°C = 298 K).For the given reaction, n = 2, so:K_eq = e^{2(0.12 V)/(8.314 J/mol·K)(298 K)} = 1.1 x 10⁴Therefore, the equilibrium constant (K_eq) for the reaction is 1.1 x 10⁴.

For the Electrochemical Cell, Cd(s)| Cd2+(aq)|| Co2+(aq)| Co(s), Determine the Equilibrium

For the Electrochemical Cell, Cd(s)| Cd²⁺(aq)|| Co²⁺(aq)| Co(s), Determine the Equilibrium