Final answer:
The question asks for the equilibrium constant (K) for a reaction with a given standard electrode potential (E0). Without additional data such as temperature and the number of electrons involved, it is not possible to calculate the exact value of K. We do understand that K is related to E0 through the Nernst equation.
Step-by-step explanation:
The question relates to the equilibrium constant (K) for a given chemical reaction with a standard electrode potential (E0) of 0.28V. According to the Nernst equation and the relationship between the standard electrode potential and the equilibrium constant, we can determine K using the formula:
K = e(nFE0/RT)
where n is the number of electrons transferred in the reaction, F is the Faraday constant (approximately 96485 C/mol), R is the gas constant (8.314 J/mol*K), and T is the temperature in Kelvin. However, since the question does not provide specific values for n, R, T, or F, a numerical calculation of K cannot be provided. The question may be missing relevant data needed to carry out the calculation, or it is assumed that you are being asked a theoretical question relating to the relationship between electrode potential and equilibrium constant.