The equilibrium constant for the reaction agbr(s) picture ag+(aq) + br− (aq) is the solubility product constant, ksp = 7.7 × 10−13 at 25°c. calculate δg for the reaction when [ag+] = 1.0 × 10−2 m and [br-] = 1.0 × 10−3 m. is the reaction spontaneous or nonspontaneous at these concentrations?

The reaction will be  non spontaneous at these concentrations.

Explanation:

Expression for an equilibrium constant :

Solubility product of the reaction:

Reaction between Gibb's free energy and equilibrium constant if given as:

Gibb's free energy when concentration and

Reaction quotient of an equilibrium = Q

Since ,the value of Gibbs free energy is greater than zero which means reaction will be non spontaneous at these concentrations

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explanation:

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