Q45.The solubility of N2 in water at 300 K and 500 torr partial pressure is 0 .01 g L−1. The solubility (in g L−1 ) at 750 torr partial pressure is: (1) 0.0075 (2) 0.005 (3) 0. 02 (4) 0.015
What This Question Tests
This question applies Henry's Law to calculate the solubility of a gas (N2) in water at a new partial pressure, given its solubility at another partial pressure and constant temperature.
Concepts Tested
Formulas Used
Solubility ∝ Partial Pressure
S₁/P₁ = S₂/P₂
📚 NCERT Sections This Tests
1.35 — Henry’S Law Constant For The Molality Of Methane In Benzene At 298 K Is
Chemistry Class 11 · Chapter 1
1.35 Henry’s law constant for the molality of methane in benzene at 298 K is 4.27 × 105 mm Hg. Calculate the solubility of methane in benzene at 298 K under 760 mm Hg.
1.34 — Vapour Pressure Of Water At 293 K Is 17.535 Mm Hg. Calculate The Vapour
Chemistry Class 11 · Chapter 1
1.34 Vapour pressure of water at 293 K is 17.535 mm Hg. Calculate the vapour pressure of water at 293 K when 25 g of glucose is dissolved in 450 g of water.
1.36 — 100 G Of Liquid A (Molar Mass 140 G Mol–1) Was Dissolved In 1000 G Of Liquid B
Chemistry Class 11 · Chapter 1
1.36 100 g of liquid A (molar mass 140 g mol–1) was dissolved in 1000 g of liquid B (molar mass 180 g mol–1). The vapour pressure of pure liquid B was found to be 500 torr. Calculate the vapour pressure of pure liquid A and its vapour pressure in the solution if the total vapour pressure of the solution is 475 Torr. 29 Solutions Reprint 2025-26
📋 Question Details
- Chapter
- Solutions
- Topic
- Henry's Law
- Year
- 2016
- Shift
- 09 Apr Online
- Q Number
- Q45
- Type
- MCQ
- NCERT Ref
- Class 12 Chemistry Ch 2: Solutions
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