Hydrogen iodide, HI, is used as a reagent in organic chemistry to transform primary alcohols into alkyl iodides. Suppose you are a chemist using HI; you would need to understand the equilibrium behavior of HI to maximize your yield of products. At 25.00°C, the standard Gibbs free energy of reaction for 1/2H₂(g) + 1/2 I₂(s) → HI(g) is 11.70 kJ · mol^–1; calculate the equilibrium constant for this reaction.

ANTICIPATE Because the standard Gibbs free energy of the reaction is positive, you should expect the equilibrium constant to be less than 1.

PLAN Use Eq. 7 with the temperature in kelvins.

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AGO - RT In K = (7)