For a reaction with a H^o = +50 kJ and a $\Delta$S^o = +100.0 J/K,$\Delta$G^o is____________________ and the equilibrium constant is____________________ .

Question

Quizplus · Accepted Answer

The Gibbs free energy change ($\Delta G$) can be calculated using the equation $\Delta G = \Delta H - T\Delta S$, where $\Delta H$ is the enthalpy change, $T$ is the temperature in Kelvin, and $\Delta S$ is the entropy change. Given $\Delta H = +50 kJ = +50000 J$ (since 1 kJ = 1000 J) and $\Delta S = +100.0 J/K$, without the specific temperature $T$ provided, we can't calculate the exact value of $\Delta G$. However, since both $\Delta H$ and $\Delta S$ are positive, at any temperature, the term $T\Delta S$ will also be positive, potentially making $\Delta G$ either positive or negative depending on the magnitude of $T\Delta S$ compared to $\Delta H$. Yet, the question seems to imply a single answer regarding $\Delta G$ and the equilibrium constant, which might be an oversight or simplification for theoretical discussion.In general, if $\Delta G$ is positive, the reaction is non-spontaneous, and the equilibrium constant $K$ is less than 1, indicating that reactants are favored at equilibrium. This aligns with choice C. However, it's important to note that the actual sign of $\Delta G$ depends on the temperature due to the $T\Delta S$ term, and without specifying temperature, a definitive calculation of $\Delta G$ and determination of the equilibrium constant's magnitude is not possible. The answer provided is based on the general understanding that a positive $\Delta H$ and a positive $\Delta S$ can lead to either a positive or negative $\Delta G$ depending on the temperature, but typically, a positive $\Delta H$ suggests that the process might require input of energy (making it less likely to be spontaneous at lower temperatures), and the positive $\Delta S$ suggests that the disorder is increasing, which could favor spontaneity at higher temperatures. The equilibrium constant's relation to $\Delta G$ is given by the equation $K = e^{-\Delta G/RT}$, where $R$ is the gas constant and $T$ is the temperature in Kelvin. Without specific temperature values, the precise relationship between $\Delta G$ and $K$ cannot be accurately determined from the given data.

For a Reaction with a Ho = +50 KJ and A \Delta

For a Reaction with a H^o = +50 KJ and A \Delta