💨2 Effect of Pressure on Solubility of Gases in Liquids

 Absolutely, Mayank! Here's a simplified, impactful, and CBSE Class 12 board exam–oriented explanation of the Effect of Pressure on Solubility of Gases in Liquids, perfectly structured for classroom presentation or revision slides:

💨 Effect of Pressure on Solubility of Gases in Liquids

📚 CBSE Class 12 | Easy | Exam-Focused

✅ Key Idea:

The solubility of a gas in a liquid increases with an increase in pressure.

🧪 Why Does This Happen? (Simple Explanation)

  • Gases are compressible.

  • When pressure increases, more gas particles are forced into the liquid.

  • This increases the rate of gas molecules entering the solution.

  • Eventually, a new dynamic equilibrium is reached — with more gas dissolved.

⚖️ Dynamic Equilibrium:

Gas (above liquid)⇌Gas (dissolved in liquid)\text{Gas (above liquid)} \rightleftharpoons \text{Gas (dissolved in liquid)}

📌 At high pressure: More gas moves into the liquid
📌 At low pressure: More gas escapes out of the liquid

🧠 Henry’s Law (Very Important for Boards)

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

🧮 Henry’s Law Formula:

p=KH⋅xp = K_H \cdot x

Where:

  • p = partial pressure of gas

  • x = mole fraction of gas in solution

  • KH = Henry’s constant (depends on gas & temperature)

📌 Important Points to Remember:

Condition Effect on Solubility
↑ Pressure ↑ Solubility
↑ Temperature ↓ Solubility
↑ KH value ↓ Solubility

🔍 Why KH Matters?

  • Each gas has a different KH value.

  • Higher KH means the gas is less soluble.

  • Example from data:

    • CO₂ has low KH → dissolves easily (used in soda)

    • He has high KH → very low solubility

📘 Applications of Henry’s Law (CBSE Must-Know)

Application Explanation
Soda/Soft Drinks CO₂ is dissolved under high pressure
Scuba Diving High pressure dissolves N₂ in blood; sudden pressure drop → nitrogen bubbles → bends
High Altitudes Low O₂ pressure → less oxygen dissolves in blood → anoxia (weakness, dizziness)

📝 CBSE Exam Tips:

✅ Define Henry’s Law clearly
✅ Write the formula p = K_H × x
✅ Give 2 real-life examples
✅ Mention pressure increases solubility

Would you like this as:

  • 📊 A PowerPoint slide deck

  • 📄 A PDF handout for students

  • 🧠 Or a chalkboard-style summary image?

I can make any of these formats for your next class!Absolutely, Mayank! Here's a simplified, impactful, and CBSE Class 12 board exam–oriented explanation of the Effect of Pressure on Solubility of Gases in Liquids, perfectly structured for classroom presentation or revision slides:

💨 Effect of Pressure on Solubility of Gases in Liquids

📚 CBSE Class 12 | Easy | Exam-Focused

✅ Key Idea:

The solubility of a gas in a liquid increases with an increase in pressure.

🧪 Why Does This Happen? (Simple Explanation)

  • Gases are compressible.

  • When pressure increases, more gas particles are forced into the liquid.

  • This increases the rate of gas molecules entering the solution.

  • Eventually, a new dynamic equilibrium is reached — with more gas dissolved.

⚖️ Dynamic Equilibrium:

Gas (above liquid)⇌Gas (dissolved in liquid)\text{Gas (above liquid)} \rightleftharpoons \text{Gas (dissolved in liquid)}

📌 At high pressure: More gas moves into the liquid
📌 At low pressure: More gas escapes out of the liquid

🧠 Henry’s Law (Very Important for Boards)

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

🧮 Henry’s Law Formula:

p=KH⋅xp = K_H \cdot x

Where:

  • p = partial pressure of gas

  • x = mole fraction of gas in solution

  • KH = Henry’s constant (depends on gas & temperature)

📌 Important Points to Remember:

Condition Effect on Solubility
↑ Pressure ↑ Solubility
↑ Temperature ↓ Solubility
↑ KH value ↓ Solubility

🔍 Why KH Matters?

  • Each gas has a different KH value.

  • Higher KH means the gas is less soluble.

  • Example from data:

    • CO₂ has low KH → dissolves easily (used in soda)

    • He has high KH → very low solubility

📘 Applications of Henry’s Law (CBSE Must-Know)

Application Explanation
Soda/Soft Drinks CO₂ is dissolved under high pressure
Scuba Diving High pressure dissolves N₂ in blood; sudden pressure drop → nitrogen bubbles → bends
High Altitudes Low O₂ pressure → less oxygen dissolves in blood → anoxia (weakness, dizziness)

📝 CBSE Exam Tips:

✅ Define Henry’s Law clearly
✅ Write the formula p = K_H × x
✅ Give 2 real-life examples
✅ Mention pressure increases solubility

Would you like this as:

  • 📊 A PowerPoint slide deck

  • 📄 A PDF handout for students

  • 🧠 Or a chalkboard-style summary image?

I can make any of these formats for your next class!

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