For the reaction below ΔG° = +33.0 kJ,ΔH° = +92.2 kJ,and ΔS° = +198.7 J/K.Estimate the temperature at which this reaction becomes spontaneous. 2 NH₃(g)→ N₂(g)+ 3 H₂(g)

Question

Quizplus · Accepted Answer

To determine the temperature at which the reaction becomes spontaneous, we use the equation:
ΔG = ΔH - TΔS
For a spontaneous reaction, ΔG < 0
So, we can rearrange the equation as:
T = ΔH/ΔS - ΔG/ΔS
Substitute the given values:
T = (92.2 kJ) / (198.7 J/K) - (-33.0 kJ) / (198.7 J/K) = 463.7 K ≈ 464 K
Therefore, the temperature at which this reaction becomes spontaneous is approximately 464 K. The correct answer is D.

For the Reaction Below ΔG° = +33