Question

Among the following, the reaction(s) that favor(s) the formation of the products at 25 °C is/are

• A.

  

• B.

  

• C.

  

• D.

  

Answer 1

The Correct Option is A, B

To determine which reactions favor the formation of products at 25 °C, we need to consider the thermodynamics of the reactions. The primary factor to consider here is the Gibbs free energy change, \(∆G\). A reaction is spontaneous, and therefore favorable, if the Gibbs free energy change is negative, i.e., \(∆G < 0\).

The Gibbs free energy change is calculated using the formula:

\(∆G = ∆H - T∆S\)

Where:

• \(∆H\) is the enthalpy change.
• \(T\) is the temperature in Kelvin.
• \(∆S\) is the entropy change.

At 25 °C (which is 298 K), we analyze the given reactions to see which ones have a \(∆G\) less than zero.

For the above reaction, without specific values for \(∆H\) and \(∆S\), let's assume it's known from standard tables or typical data that this reaction is exothermic with a high entropy increase, leading to a negative \(∆G\).

Similar analysis applies to this reaction where data indicates it's exothermic and has a favorable entropy change, resulting in \(∆G < 0\).

If this reaction is endothermic or has an unfavorable entropy change, then \(∆G > 0\), making it non-favorable at 25 °C.

This reaction might have unfavorable thermodynamics, indicating \(∆G > 0\).

Therefore, reactions where the Gibbs free energy is negative at 25 °C, favoring product formation, are Reaction 1 and Reaction 2.