Question

1 Point
For a reaction, a H= 198 kJ. For which value of TA Sis the reaction
spontaneous?
O A. -198 kJ
O B. 198 kJ
O C. Oku
O D. 396 kJ
SUBMIT

Answer 1

The correct answer is D. 396 kJ. ΔG will be negative for this value of TΔS indicating a spontaneous reaction.

Further Explanation:

• The value of the Gibbs Free Energy (ΔG) determines the spontaneity of the reaction.
• To get this value, an equation than shows the relationship among the Gibbs Free Energy (ΔG), enthalpy (ΔH), entropy (ΔS), and temperature is used: $dG \ = dH \ - TdS$
• A positive ΔG represents a non-spontaneous reaction
• A negative ΔG value indicates a spontaneous reaction.

A. -198 kJ FALSE because this gives a positive ΔG.

$dG \ = \ 198 \ kJ \ - \ (-198 \ kJ) \\\boxed {dG = 396 \ kJ}$

B. 198 kJ FALSE because this results in ΔG = 0. The reaction is at equilibrium.

$dG \ = \ 198 \ kJ \ - \ 198 \ kJ \\\boxed {dG = 0}$

C. 0 kJ FALSE because this results in a positive ΔG.

$dG = 198 \ kJ \ - \ 0\\\boxed {dG = 198 \ kJ}$

D. 396 kJ TRUE because this results in a negative ΔG.

$dG = \ 198 \ kJ \ - \ 396 \ kJ\\\boxed {dG = -198 \ kJ}$

Learn More

1. Learn more about enthalpy https://brainly.com/question/1127247
2. Learn more about entropy https://brainly.com/question/490678
3. Learn more about Gibbs Free Energy  https://brainly.com/question/9552459

Keywords: Gibbs Free Energy, spontaneity