For a particular reaction at 298 K, the equilibrium constant is equal to 581. Determine ΔG° in kJ/mol for the reaction. Do not include units. Report your answer to 3 significant figures.

The standard Gibbs free energy of the reaction is -15.8 kJ/mol

Explanation:

Relation between standard Gibbs free energy and equilibrium constant follows:

where,

= Standard Gibbs free energy = ?

R = Gas constant =

T = temperature = 298 K

 = equilibrium constant = 581

Putting values in above equation, we get:

Conversion factor used: 1 kJ = 1000 J

Hence, the standard Gibbs free energy of the reaction is -15.8 kJ/mol

why do the isotopes of a particular element behave differently in nuclear reactions but the same in chemical reactions? chemical reactions involve changes to electrons in an atom; isotopes do not differ in electrons, and so they react the same way during chemical changes.

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