# Why is the equilibrium constant for a Daniell cell not equal 1?

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?

• 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. – MaxW Feb 26 at 5:30