$\Delta$ G° = -53.6 kJ/mol_rxn for the following reaction at 25°C.
Zn²⁺(aq) + 4 NH₃(aq) $\rightarrow$ Zn(NH₃) ₄²⁺(aq)
What is the value of the complex formation equilibrium constant for this reaction?

Question

\Delta

G° = -53.6 kJ/mol_rxn for the following reaction at 25°C.
Zn²⁺(aq) + 4 NH₃(aq)

\rightarrow

Zn(NH₃) ₄²⁺(aq)
What is the value of the complex formation equilibrium constant for this reaction?

Quizplus · Accepted Answer

The complex formation equilibrium constant is given by the equation:K = e^(-ΔG°/RT)where ΔG° is the standard free energy change, R is the gas constant (8.314 J/mol·K), and T is the temperature in Kelvin (25°C = 298 K).Plugging in the values given in the question, we get:K = e^(-(-53.6 kJ/mol)/(8.314 J/mol·K)(298 K)) = 2.5 x 10^9

Δ\DeltaΔ G° = -536 KJ/molrxn for the Following Reaction at 25°C

$\Delta$ G° = -536 KJ/mol_rxn for the Following Reaction at 25°C