Consider the gibbs energies at 25 ∘ c. substance δ∘f (kj·mol−1) ag (aq) 77. 1 cl−(aq) −131. 2 agcl(s) −109. 8 br−(aq) −104. 0 agbr(s) −96. 9 (a) calculate δ∘rxn for the dissolution of agcl(s)

The gibbs free energy is termed as thermodynamic quantity which is equal to the enthalpy (of a system or process) subtracted by the product of the entropy and the absolute temperature.

The gibbs free energy of the reaction is given by:

∆G°(rxn) =sum of ([∆G°] products)- sum of ( [∆ G°] reactants)

Reaction can be given as:

AgCl(S) » Ag+ (aq) + Cl- (aq)

Gibbs free energy of silver ions = ∆G°f, (Ag+) = 77.1kJ/mol

Gibbs free energy of formation of chloride ions = ∆G°f, (Cl-)= -131. 2kJ/mol

Gibbs free energy of formation of silver chloride solid = ∆ G°f, (AgCl) = - 109.8kJ/mol

The gibbs free energy of the reaction of dissolution of AgCl) :∆ G°rxn:

∆G°rxn = (77.1kJ/mol) – (- 109.8kJ/mol)

55.7kJ/mol

Thus, we found that the ∆G° for the dissolution of AgCL solid is 55.7 kJ/mol.

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