Consider the reaction of 25.0 mL of 0.20 M AgNO₃(aq)with 25.0 mL of 0.20 M NaBr(aq)to form AgBr(s)at 25 °C.What is ΔG for this reaction? The K_sp of AgBr is 5.0 × 10^-13 at 25 °C. A)-58.8 kJ/mol B)-70.2 kJ/mol C)+58.8 kJ/mol D)+70.2 kJ/mol E)-28.3 kJ/mol

Question

Quizplus · Accepted Answer

The equation for the reaction is:

AgNO3(aq) + NaBr(aq) → AgBr(s) + NaNO3(aq)

The reaction quotient Qc can be calculated as follows:

Qc = [AgBr]/([AgNO3]*[NaBr])

Substituting the given values:

Qc = [AgBr]/(0.20*0.025)^2

Qc = [AgBr]/1.25×10^-6

At equilibrium, Qc = Ksp, therefore:

Ksp = [AgBr]/1.25×10^-6

[AgBr] = Ksp * 1.25×10^-6

[AgBr] = 5.0×10^-13 * 1.25×10^-6

[AgBr] = 6.25×10^-19

The change in Gibbs free energy can be calculated using the formula:

ΔG = -RTlnK

Substituting the given values:

ΔG = -(8.314 J/mol*K) * (298 K) * ln(6.25×10^-19)

ΔG = -58.8 kJ/mol

Therefore, the correct answer is A) -58.8 kJ/mol.

Consider the Reaction of 25