Question

When the elements react to form compounds, a negative free energy change (\(\Delta G\)) means

(A) Spontaneous reaction
(B) Free energy of the products is higher than that of reactants
(C) Very high activation barrier
(D) Exergonic reactions
Choose the correct answer from the options given below:

• A. (A), (B) and (D) only.
• B. (A), (B) and (C) only.
• C. (A), (B), (C) and (D).
• D. (A) and (D) only.

Hint:

A negative \(\Delta G\) indicates a spontaneous, exergonic reaction where energy is released.

Answer 1

The Correct Option is D

Step 1: Free energy change (\(\Delta G\)) in reactions.
- A negative \(\Delta G\) signifies a spontaneous reaction that occurs without needing external energy.
- Spontaneous reactions proceed in the direction of decreasing free energy.
- Exergonic reactions, which release energy, are characterized by a negative \(\Delta G\).
- Option (B) is wrong; a negative \(\Delta G\) means the products have lower, not higher, free energy than the reactants.
- Option (C): Spontaneous reactions can have high activation energy, but it's not a requirement for a negative \(\Delta G\).
Step 2: Conclusion. Therefore, the correct options relate to spontaneous and exergonic reactions.
Final Answer: \[ \boxed{\text{(A) and (D) only}} \]