Question

question 12 of 30
for a reaction, $\delta h = 198$ kj. for which value of $t\delta s$ is the reaction spontaneous?

a. 396 kj

b. 198 kj

c. -198 kj

d. 0 kj

Explanation:

Step1: Recall spontaneity condition

For a reaction to be spontaneous, the Gibbs free energy change \(\Delta G\) must be negative. The formula for \(\Delta G\) is \(\Delta G=\Delta H - T\Delta S\).

Step2: Substitute \(\Delta H\) and analyze

Given \(\Delta H = 198\space kJ\). We need \(\Delta G<0\), so \(198 - T\Delta S<0\), which implies \(T\Delta S>198\space kJ\).
Looking at the options, only option A (\(396\space kJ\)) is greater than \(198\space kJ\).

Answer:

A. 396 kJ