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

atomic number of carbon is 6

electronic configuration of carbon is 1s²2s²2p²

orbital diagram of carbon is as shown here in the image.

idk i’m struggling too