The spontaneity of a reaction is determined by the Gibbs Free Energy equation, which is ΔG = ΔH - TΔS. For a reaction to be spontaneous, ΔG must be less than 0.

Given that ΔH = 198 kJ, we can rearrange the equation to solve for TΔS:

TΔS = ΔH - ΔG

Since we want ΔG to be less than 0 for spontaneity, we can set ΔG to be 0 for the threshold of spontaneity:

TΔS = ΔH - 0
TΔS = 198 kJ

Therefore, for the reaction to be spontaneous, TΔS must be greater than 198 kJ. So, the correct answer is B. 396 kJ.

Question

The spontaneity of a reaction is determined by the Gibbs Free Energy equation, which is ΔG = ΔH - TΔS. For a reaction to be spontaneous, ΔG must be less than 0.

Given that ΔH = 198 kJ, we can rearrange the equation to solve for TΔS:

TΔS = ΔH - ΔG

Since we want ΔG to be less than 0 for spontaneity, we can set ΔG to be 0 for the threshold of spontaneity:

TΔS = ΔH - 0
TΔS = 198 kJ

Therefore, for the reaction to be spontaneous, TΔS must be greater than 198 kJ. So, the correct answer is B. 396 kJ.

Knowee AI · Accepted Answer

The spontaneity of a reaction is determined by the Gibbs Free Energy equation, which is ΔG = ΔH - TΔS. For a reaction to be spontaneous, ΔG must be less than 0.

Given that ΔH = 198 kJ, we can rearrange the equation to solve for TΔS:

TΔS = ΔH - ΔG

Since we want ΔG to be less than 0 for spontaneity, we can set ΔG to be 0 for the threshold of spontaneity:

TΔS = ΔH - 0
TΔS = 198 kJ

Therefore, for the reaction to be spontaneous, TΔS must be greater than 198 kJ. So, the correct answer is B. 396 kJ.

For a reaction, H = 198 kJ. For which value of TS is the reaction spontaneous?A.0 kJB.396 kJC.-198 kJD.198 kJ

Question

For a reaction, H = 198 kJ. For which value of TS is the reaction spontaneous?

Solution

Similar Questions

Upgrade your grade with Knowee