At the equilibrium position in the process of adsorption …………

Options

A. `Delta H gt 0`
B. `Delta H=T Delta S`
C. `Delta H gt T Delta S`
D. `Delta H lt T Delta S`

Explanation

To solve the question regarding the equilibrium position in the process of adsorption, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Concept of Adsorption**:
- Adsorption is defined as the accumulation of molecular species at the surface of a solid rather than in the bulk of the solid. This process involves the adhesion of atoms, ions, or molecules from a gas, liquid, or dissolved solid to a surface.

2. **Identify the Nature of the Adsorption Process**:
- The adsorption process is generally exothermic, meaning it releases heat. This can be represented as:
\[ \Delta H < 0 \]
where \(\Delta H\) is the change in enthalpy.

3. **Apply Thermodynamic Principles**:
- The relationship between Gibbs free energy (\(\Delta G\)), enthalpy (\(\Delta H\)), temperature (T), and entropy (\(\Delta S\)) is given by the equation:
\[ \Delta G = \Delta H - T \Delta S \]

4. **Consider the Equilibrium Condition**:
- At equilibrium, the Gibbs free energy change (\(\Delta G\)) is zero:
\[ \Delta G = 0 \]
Therefore, substituting into the equation gives:
\[ 0 = \Delta H - T \Delta S \]

5. **Derive the Relationship at Equilibrium**:
- Rearranging the equation leads to:
\[ \Delta H = T \Delta S \]
This indicates that at equilibrium, the change in enthalpy is equal to the product of temperature and the change in entropy.

### Final Answer:
At the equilibrium position in the process of adsorption, we have:
\[ \Delta H = T \Delta S \]