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Using the equation

$$RT\ln K = nFE,$$

the equilibrium constant $K$ for a Daniell cell at standard conditions can be found as

$$K = \exp\left(\frac{2 × 96500 × 1.1}{8.3145 × 298.15}\right) = \pu{1.55E37}$$

However since we know that $K$ equals the ratio of the concentration of the products to that of the reactants, then we find $K = 1$ at standard conditions. So, where did I go wrong because I know both explanations are right?

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    $\begingroup$ That "K = 1 at standard conditions" is wrong. The voltage for a "standard" Daniel Cell is 1.10 V which indicates that a reaction will be spontaneous when the two half-cells are connected. $\endgroup$ – MaxW Feb 26 at 5:30

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