Question

at 298 k, $delta h^{0}=46$ kj/mol and $delta s^{0}=0.097$ kj/(k·mol). what is the gibbs free energy of the reaction?

a. 1300 kj
b. 75 kj
c. 0.63 kj
d. 17 kj

Explanation:

Step1: Recall Gibbs - free energy formula

The formula for Gibbs - free energy is $\Delta G=\Delta H - T\Delta S$.

Step2: Substitute the given values

We are given that $\Delta H = 46\ kJ/mol$, $T = 298\ K$, and $\Delta S=0.097\ kJ/(K\cdot mol)$.
Substitute these values into the formula: $\Delta G=46 - 298\times0.097$.
First, calculate $298\times0.097 = 29.906$.
Then, $\Delta G=46 - 29.906$.

Step3: Calculate the result

$\Delta G = 16.094\approx17\ kJ/mol$.

Answer:

D. 17 kJ