Calculate the Gibbs free energy of the reaction from mixing 50 mL each of 0.50 M AgNO3(aq) solution and 1 M of NaCl(aq) to form AgCl(s) at 25°. The Ksp of AgCl is 6.0 × 10—11 at 25 °C.

To calculate the Gibbs free energy (ΔG) of the reaction, we first need to find the equilibrium constant (K) of the reaction. The reaction is:

AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3(aq)

Since AgCl is a solid, its concentration is not included in the equilibrium expression. The Ksp given is for the dissolution of AgCl, which is the reverse of the reaction given. So, the equilibrium constant for the reaction given is the reciprocal of the Ksp, which is 1/(6.0 × 10^-11) = 1.67 x 10^10.

Next, we use the formula for Gibbs free energy:

ΔG = -RTlnK

where R is the gas constant (8.314 J/(mol·K)) and T is the temperature in Kelvin. Converting 25°C to Kelvin gives