Consider the following hypothetical reaction (at 308 K). Standard free energies, in kJ/mol, are given in parentheses. What is the value of the equilibrium constant for the reaction at 308 K?

Question

Consider the following hypothetical reaction (at 308 K). Standard free energies, in kJ/mol, are given in parentheses.  What is the value of the equilibrium constant for the reaction at 308 K?

Quizplus · Accepted Answer

The equilibrium constant, K, can be calculated using 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.

Converting the given standard free energies to Joules and plugging them into the equation, we get:

K = e^(-(45,000 J/mol)/(8.314 J/mol*K * 308 K))
K = e^(-17.9)

Using a calculator or logarithm tables, we find:

K = 0.28

Therefore, the answer is B.

Consider the Following Hypothetical Reaction (At 308 K)