💨 Effect of Pressure on Solubility of Gases in Liquids

 Here’s a CBSE Class 12–oriented explanation of the paragraph you provided, presented in a student-friendly, simplified format—perfect for classroom teaching, notes, or slides.

💨 Effect of Pressure on Solubility of Gases in Liquids

✅ Key Concept:

Solubility of a gas in a liquid increases with increase in pressure.

🔬 How Does It Work?

  • Consider a container with gas above a liquid at pressure p and temperature T.

  • Gas molecules are constantly moving — some enter the liquid (dissolution), while others leave (escape).

📌 At dynamic equilibrium, the rate of gas entering = rate of gas leaving the solution.

🔺 Now Increase the Pressure:

  • By compressing the gas, we increase the number of gas particles per unit volume.

  • More gas molecules hit the liquid surface → more gas dissolves into the liquid.

  • A new equilibrium is established, but now with higher gas solubility.

⚖️ Henry’s Law – Explains the Relationship

At constant temperature, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.

🧪 Mathematical Form:

p=KH⋅xp = K_H \cdot x

Where:

  • p = partial pressure of the gas above the solution

  • x = mole fraction of gas in the solution

  • KH = Henry’s law constant (depends on the gas and temperature)

📈 Graph:

A straight-line graph is obtained when we plot:

  • p (y-axis) vs x (x-axis)
    ➝ Slope = KH

📌 Important Observations:

  • Different gases have different KH values.

  • Higher KH = Lower solubility of gas.

  • KH increases with temperature, so solubility of gas decreases as temperature rises.

📝 Example (from Table):

Gas Temp (K) KH (kbar) Solubility
CO₂ 298 1.67 High
O₂ 293 34.86 Moderate
N₂ 293 76.48 Low
He 293 144.97 Very Low

🧠 Summary:

Factor Effect on Gas Solubility
↑ Pressure ↑ Solubility
↑ Temperature ↓ Solubility
↑ KH value ↓ Solubility

✅ CBSE Exam Tip:

  • Always define Henry’s Law clearly and write the formula:

    p=KH⋅xp = K_H \cdot x

  • Mention dynamic equilibrium, molecular collisions, and applications.

Would you like a diagram or animation-style slide content showing gas pressure and dissolution?

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