The equilibrium `H_(2) O (l) hArr H_(2)O (v) " is attained in a closed container at "40^(@)C.` The aqueous tension of water at `40^(@)C " is 23 mm . What is " K_(p)` for the said equilibrium ?

Explanation

To find the equilibrium constant \( K_p \) for the reaction \( H_2O (l) \rightleftharpoons H_2O (v) \) at 40°C, we can follow these steps:

### Step 1: Understand the Equilibrium
The equilibrium we are dealing with involves the conversion of liquid water to water vapor. In a closed container, both phases can coexist, and we can measure the pressure exerted by the vapor.

### Step 2: Identify the Aqueous Tension
The problem states that the aqueous tension (also known as vapor pressure) of water at 40°C is 23 mmHg. This value represents the pressure exerted by the water vapor when the system is in equilibrium.

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