To accurately match thermodynamic parameters from List I with their descriptions in List II, we use the Gibbs free energy equation: \[ \Delta G = \Delta H - T \Delta S \] Where:
- \( \Delta G \): Gibbs free energy change
- \( \Delta H \): Enthalpy change
- \( \Delta S \): Entropy change
- \( T \): Temperature (Kelvin)
Reaction spontaneity is determined by the sign of \( \Delta G \):
- \( \Delta G < 0 \): Spontaneous reaction
- \( \Delta G > 0 \): Non-spontaneous reaction
Temperature's effect on spontaneity depends on the signs of \( \Delta H \) and \( \Delta S \):
- Exothermic (\( \Delta H < 0 \)) and Decreasing Entropy (\( \Delta S < 0 \)):
- Spontaneous at low temperatures.
- Non-spontaneous at high temperatures. - Exothermic (\( \Delta H < 0 \)) and Increasing Entropy (\( \Delta S > 0 \)):
- Spontaneous at all temperatures. - Endothermic (\( \Delta H > 0 \)) and Increasing Entropy (\( \Delta S > 0 \)):
- Spontaneous at high temperatures.
- Non-spontaneous at low temperatures. - Endothermic (\( \Delta H > 0 \)) and Decreasing Entropy (\( \Delta S < 0 \)):
- Non-spontaneous at all temperatures.
We will now analyze each item in List I and match it to its corresponding description in List II.
- List I Item A: \( \Delta H = -\text{ve}, \Delta S = -\text{ve}, \Delta G = -\text{ve} \)
Interpretation: \[ \Delta G = \Delta H - T \Delta S = (-) - T(-) = -\text{ve} + T\Delta S \] - With \( \Delta H < 0 \) and \( \Delta S < 0 \), the reaction is spontaneous (\( \Delta G < 0 \)) at low temperatures and non-spontaneous (\( \Delta G > 0 \)) at high temperatures.
- Matching Description: Spontaneous at low temperature.
- Corresponding List II Item: III. Reaction will be spontaneous at low temperature. - List I Item B: \( \Delta H = -\text{ve}, \Delta S = -\text{ve}, \Delta G = +\text{ve} \)
Interpretation: \[ \Delta G = \Delta H - T \Delta S = (-) - T(-) = -\text{ve} + T\Delta S \] - Given \( \Delta G > 0 \), the reaction is non-spontaneous.
- Since \( \Delta H < 0 \) and \( \Delta S < 0 \), the reaction becomes non-spontaneous at high temperatures.
- Matching Description: Non-spontaneous at high temperature.
- Corresponding List II Item: I. Reaction will be non-spontaneous at high temperature. - List I Item C: \( \Delta H = +\text{ve}, \Delta S = +\text{ve}, \Delta G = +\text{ve} \)
Interpretation: \[ \Delta G = \Delta H - T \Delta S = (+) - T(+) \] - Given \( \Delta G > 0 \), the reaction is non-spontaneous.
- With \( \Delta H > 0 \) and \( \Delta S > 0 \), the reaction is non-spontaneous at low temperatures, becoming spontaneous at high temperatures.
- Matching Description: Spontaneous at high temperature.
- Corresponding List II Item: IV. Reaction will be spontaneous at high temperature. - List I Item D: \( \Delta H = +\text{ve}, \Delta S = +\text{ve}, \Delta G = -\text{ve} \)
Interpretation: \[ \Delta G = \Delta H - T \Delta S \] - With \( \Delta H > 0 \) and \( \Delta S > 0 \), the reaction is spontaneous at high temperatures and non-spontaneous at low temperatures.
- Matching Description: Non-spontaneous at low temperature.
- Corresponding List II Item: II. Reaction will be non-spontaneous at low temperature.
Summary of Matches:
\[ \text{(A)} \, -\Delta H, -\Delta S, -\Delta G \rightarrow \text{III. Spontaneous at low temp} \\ \text{(B)} \, -\Delta H, -\Delta S, +\Delta G \rightarrow \text{I. Non-spontaneous at high temp} \\ \text{(C)} \, +\Delta H, +\Delta S, +\Delta G \rightarrow \text{II. Non-spontaneous at low temp} \\ \text{(D)} \, +\Delta H, +\Delta S, -\Delta G \rightarrow \text{IV. Spontaneous at high temp} \] Therefore, the correct matches are:
\[ \boxed{\text{(A) - (III), (B) - (I), (C) - (II), (D) - (IV)}} \]