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प्रश्न
State Henry’s law and explain why are the tanks used by scuba divers filled with air diluted with helium (11.7% helium, 56.2% nitrogen and 32.1% oxygen)?
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उत्तर
Henry’s law: the partial pressure of the gas in vapour phase (p) is proportional to the mole fraction of the gas (x) in the solution.
The pressure underwater is high, so the solubility of gases in blood increases. When the diver comes to surface the pressure decreases so does the solubility causing bubbles of nitrogen in blood, to avoid this situation and maintain the same partial pressure of nitrogen underwater too, the dilution is done.
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संबंधित प्रश्न
Gas (A) is more soluble in water than Gas (B) at the same temperature. Which one of the two gases will have the higher value of KH (Henry’s constant) and why
Why do gases always tend to be less soluble in liquids as the temperature is raised?
Based on solute-solvent interactions, arrange the following in order of increasing solubility in n-octane and explain.
Cyclohexane, KCl, CH3OH, CH3CN
A solution is prepared by dissolving 9.25 g of non-volatile solute in 450 mL of water. It has an osmotic pressure of 350 mm of Hg at 27°C. Assuming the solute is non-electrolyte, determine its molecular mass. (R = 0.0821 Lit-atm K−1 mol−1)
State Henry’s law.
Henry’s law constant of oxygen is 1.4 × 10–3 mol lit–1 atm–1 at 298 K. How much of oxygen is dissolved in 100 ml at 298 K when the partial pressure of oxygen is 0.5 atm?
The value of Henry's constant KH is ______.
Solubility of gases in liquids decreases with rise in temperature because dissolution is an ______.
What is the significance of Henry’s Law constant KH?
Assertion (A): Helium is used to dilute oxygen in diving apparatus.
Reason (R): Helium has high solubility in O.
In the light of the above statements, choose the correct answer from the options given below:
