Question

The favourable conditions for a spontaneous reaction are:

• A. \( T \Delta S>\Delta H \), \( \Delta H = + \), \( \Delta S = + \)
• B. \( T \Delta S>\Delta H \), \( \Delta H = + \), \( \Delta S = - \)
• C. \( T \Delta S>\Delta H \), \( \Delta H = - \), \( \Delta S = - \)
• D. \( T \Delta H = \Delta S \), \( \Delta H = + \), \( \Delta S = + \)

Hint:

For spontaneity, \( T \Delta S>\Delta H \), ensuring that the free energy is negative.

Answer 1

The Correct Option is A

Step 1: Understand the spontaneity conditions.
A spontaneous reaction must have a positive \( \Delta S \) and \( T \Delta S>\Delta H \). This ensures that the free energy is negative, indicating spontaneity.
Step 2: Conclusion.
Thus, the favourable conditions are \( T \Delta S>\Delta H \), \( \Delta H = + \), \( \Delta S = + \).
Final Answer: \[ \boxed{A} \]