Assume that the reaction Occurs in an mixture of ideal gases. At 700 K, K_p = 5.10. At this temperature, what is $\Delta$G°?

Question

Quizplus · Accepted Answer

The formula for calculating the standard Gibbs free energy change ($\Delta G^\circ$) of a reaction is:

$$\Delta G^\circ = -RT\ln(K)$$

Where $R$ is the gas constant, $T$ is temperature in Kelvin, and $K$ is the equilibrium constant.

Since we are given the value of $K$, we can calculate $\Delta G^\circ$ as:

$$\Delta G^\circ = -RT\ln(5.10)$$

Plugging in the values gives:

$$\Delta G^\circ = -(8.314\,\mathrm{J/mol}\cdot\mathrm{K})(700\,\mathrm{K})\ln(5.10)$$

$$\Delta G^\circ = -9.48\,\mathrm{kJ/mol}$$

Therefore, the answer is choice (C).

Assume That the Reaction Occurs in an Mixture of Ideal